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Introduction to Chemistry

Bishop

Chapter 6

Oxidation-Reduction Reactions - all with Video Answers

Educators

Chapter Questions

00:50

Problem 1

For each of the following ionic formulas, write the formula for the cation and the formula for the anion.
a. $\mathrm{FeBr}_3$
b. $\mathrm{Co}_3\left(\mathrm{PO}_4\right)_2$
c. AgCl
d. $\left(\mathrm{NH}_4\right)_2 \mathrm{SO}_4$

Ronald Prasad
Ronald Prasad
Numerade Educator
00:47

Problem 2

Classify each of the following formulas as representing a binary ionic compound, an ionic compound with polyatomic ions, or a molecular compound.
a. $\mathrm{CF}_4$
b. $\mathrm{Pb}\left(\mathrm{C}_2 \mathrm{H}_3 \mathrm{O}_2\right)_2$
c. $\mathrm{CoCl}_2$
d. $\mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}$
e. $\mathrm{H}_2 \mathrm{~S}$
f. CIF
g. $\mathrm{Cr}(\mathrm{OH})_3$
h. $\mathrm{H}_3 \mathrm{PO}_4$

Sam Limsuwannarot
Sam Limsuwannarot
Numerade Educator
04:35

Problem 3

Balance the following equations. $\left(\mathrm{C}_8 \mathrm{H}_{18}\right.$ is a component of gasoline, and $\mathrm{P}_2 \mathrm{~S}_5$ is used to make the insecticides parathion and malathion.)
a. $\mathrm{C}_8 \mathrm{H}_{18}(l)+\mathrm{O}_2(g) \rightarrow \mathrm{CO}_2(g)+\mathrm{H}_2 \mathrm{O}(l)$
b. $\mathrm{P}_4(s)+\mathrm{S}_8(s) \rightarrow \mathrm{P}_2 \mathrm{~S}_5(s)$

Nicholas Sacco
Nicholas Sacco
Numerade Educator

Problem 4

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { carbon dioxide } \\
\text { change } & \begin{array}{l}
\text { oxidizing } \\
\text { oxidizing agent }
\end{array} \\
\text { decreases } & \text { partial } \\
\text { flow of electrons } & \text { pure element } \\
\text { gains } & \text { rarely } \\
\text { half-reactions } & \text { reduced } \\
\text { heat } & \text { reducing } \\
\text { increases } & \text { reducing agent } \\
\text { light } & \text { reduction } \\
\text { loses } & \text { sulfur dioxide } \\
\text { one } & \text { transferred } \\
\text { oxidation } & \text { two or more } \\
\text { oxidized } & \text { water }
\end{array}
$$

According to the modern convention, any chemical change in which an element _____________ electrons is called an oxidation.

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03:03

Problem 5

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { carbon dioxide } \\
\text { change } & \begin{array}{l}
\text { oxidizing } \\
\text { oxidizing agent }
\end{array} \\
\text { decreases } & \text { partial } \\
\text { flow of electrons } & \text { pure element } \\
\text { gains } & \text { rarely } \\
\text { half-reactions } & \text { reduced } \\
\text { heat } & \text { reducing } \\
\text { increases } & \text { reducing agent } \\
\text { light } & \text { reduction } \\
\text { loses } & \text { sulfur dioxide } \\
\text { one } & \text { transferred } \\
\text { oxidation } & \text { two or more } \\
\text { oxidized } & \text { water }
\end{array}
$$

According to the modern definition, any chemical change in which an element _____________ electrons is called a reduction.

Carlene Jimenez
Carlene Jimenez
Numerade Educator

Problem 6

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { carbon dioxide } \\
\text { change } & \begin{array}{l}
\text { oxidizing } \\
\text { oxidizing agent }
\end{array} \\
\text { decreases } & \text { partial } \\
\text { flow of electrons } & \text { pure element } \\
\text { gains } & \text { rarely } \\
\text { half-reactions } & \text { reduced } \\
\text { heat } & \text { reducing } \\
\text { increases } & \text { reducing agent } \\
\text { light } & \text { reduction } \\
\text { loses } & \text { sulfur dioxide } \\
\text { one } & \text { transferred } \\
\text { oxidation } & \text { two or more } \\
\text { oxidized } & \text { water }
\end{array}
$$

Electrons are _____________ found unattached to atoms. Thus, for one element or compound to lose electrons and be _____________, another element or compound must be there to gain the electrons and be _____________. In other words, _____________ (loss of electrons) must be accompanied by _____________ (gain of electrons).

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03:42

Problem 7

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { carbon dioxide } \\
\text { change } & \begin{array}{l}
\text { oxidizing } \\
\text { oxidizing agent }
\end{array} \\
\text { decreases } & \text { partial } \\
\text { flow of electrons } & \text { pure element } \\
\text { gains } & \text { rarely } \\
\text { half-reactions } & \text { reduced } \\
\text { heat } & \text { reducing } \\
\text { increases } & \text { reducing agent } \\
\text { light } & \text { reduction } \\
\text { loses } & \text { sulfur dioxide } \\
\text { one } & \text { transferred } \\
\text { oxidation } & \text { two or more } \\
\text { oxidized } & \text { water }
\end{array}
$$

Reactions in which electrons are _____________, resulting in oxidation and reduction, are called oxidation-reduction reactions.

Hailey Tomashek
Hailey Tomashek
Numerade Educator

Problem 8

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { carbon dioxide } \\
\text { change } & \begin{array}{l}
\text { oxidizing } \\
\text { oxidizing agent }
\end{array} \\
\text { decreases } & \text { partial } \\
\text { flow of electrons } & \text { pure element } \\
\text { gains } & \text { rarely } \\
\text { half-reactions } & \text { reduced } \\
\text { heat } & \text { reducing } \\
\text { increases } & \text { reducing agent } \\
\text { light } & \text { reduction } \\
\text { loses } & \text { sulfur dioxide } \\
\text { one } & \text { transferred } \\
\text { oxidation } & \text { two or more } \\
\text { oxidized } & \text { water }
\end{array}
$$

The separate oxidation and reduction equations are called _____________.

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Problem 9

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { carbon dioxide } \\
\text { change } & \begin{array}{l}
\text { oxidizing } \\
\text { oxidizing agent }
\end{array} \\
\text { decreases } & \text { partial } \\
\text { flow of electrons } & \text { pure element } \\
\text { gains } & \text { rarely } \\
\text { half-reactions } & \text { reduced } \\
\text { heat } & \text { reducing } \\
\text { increases } & \text { reducing agent } \\
\text { light } & \text { reduction } \\
\text { loses } & \text { sulfur dioxide } \\
\text { one } & \text { transferred } \\
\text { oxidation } & \text { two or more } \\
\text { oxidized } & \text { water }
\end{array}
$$

A(n) _____________ is a substance that loses electrons, making it possible for another substance to gain electrons and be reduced.

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Problem 10

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { carbon dioxide } \\
\text { change } & \begin{array}{l}
\text { oxidizing } \\
\text { oxidizing agent }
\end{array} \\
\text { decreases } & \text { partial } \\
\text { flow of electrons } & \text { pure element } \\
\text { gains } & \text { rarely } \\
\text { half-reactions } & \text { reduced } \\
\text { heat } & \text { reducing } \\
\text { increases } & \text { reducing agent } \\
\text { light } & \text { reduction } \\
\text { loses } & \text { sulfur dioxide } \\
\text { one } & \text { transferred } \\
\text { oxidation } & \text { two or more } \\
\text { oxidized } & \text { water }
\end{array}
$$

A(n) _____________ is a substance that gains electrons, making it possible for another substance to lose electrons and be oxidized.

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Problem 11

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { carbon dioxide } \\
\text { change } & \begin{array}{l}
\text { oxidizing } \\
\text { oxidizing agent }
\end{array} \\
\text { decreases } & \text { partial } \\
\text { flow of electrons } & \text { pure element } \\
\text { gains } & \text { rarely } \\
\text { half-reactions } & \text { reduced } \\
\text { heat } & \text { reducing } \\
\text { increases } & \text { reducing agent } \\
\text { light } & \text { reduction } \\
\text { loses } & \text { sulfur dioxide } \\
\text { one } & \text { transferred } \\
\text { oxidation } & \text { two or more } \\
\text { oxidized } & \text { water }
\end{array}
$$

Oxidation is defined as the complete or _____________ loss of electrons, reduction as the complete or partial gain of electrons.

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Problem 12

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { carbon dioxide } \\
\text { change } & \begin{array}{l}
\text { oxidizing } \\
\text { oxidizing agent }
\end{array} \\
\text { decreases } & \text { partial } \\
\text { flow of electrons } & \text { pure element } \\
\text { gains } & \text { rarely } \\
\text { half-reactions } & \text { reduced } \\
\text { heat } & \text { reducing } \\
\text { increases } & \text { reducing agent } \\
\text { light } & \text { reduction } \\
\text { loses } & \text { sulfur dioxide } \\
\text { one } & \text { transferred } \\
\text { oxidation } & \text { two or more } \\
\text { oxidized } & \text { water }
\end{array}
$$

Just think of oxidation numbers as tools for keeping track of the _____________ in redox reactions.

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Problem 13

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { carbon dioxide } \\
\text { change } & \begin{array}{l}
\text { oxidizing } \\
\text { oxidizing agent }
\end{array} \\
\text { decreases } & \text { partial } \\
\text { flow of electrons } & \text { pure element } \\
\text { gains } & \text { rarely } \\
\text { half-reactions } & \text { reduced } \\
\text { heat } & \text { reducing } \\
\text { increases } & \text { reducing agent } \\
\text { light } & \text { reduction } \\
\text { loses } & \text { sulfur dioxide } \\
\text { one } & \text { transferred } \\
\text { oxidation } & \text { two or more } \\
\text { oxidized } & \text { water }
\end{array}
$$

If any element undergoes a(n) _____________ of oxidation number in the course of a reaction, the reaction is a redox reaction. If an element’s oxidation number _____________ in a reaction, that element is oxidized. If an element’s oxidation number _____________ in a reaction, that element is reduced. The reactant containing the element that is oxidized is the _____________ agent. The reactant containing the element that is reduced is the _____________ agent.

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Problem 14

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { carbon dioxide } \\
\text { change } & \begin{array}{l}
\text { oxidizing } \\
\text { oxidizing agent }
\end{array} \\
\text { decreases } & \text { partial } \\
\text { flow of electrons } & \text { pure element } \\
\text { gains } & \text { rarely } \\
\text { half-reactions } & \text { reduced } \\
\text { heat } & \text { reducing } \\
\text { increases } & \text { reducing agent } \\
\text { light } & \text { reduction } \\
\text { loses } & \text { sulfur dioxide } \\
\text { one } & \text { transferred } \\
\text { oxidation } & \text { two or more } \\
\text { oxidized } & \text { water }
\end{array}
$$

In combination reactions, _____________ elements or compounds combine to form one compound.

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Problem 15

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { carbon dioxide } \\
\text { change } & \begin{array}{l}
\text { oxidizing } \\
\text { oxidizing agent }
\end{array} \\
\text { decreases } & \text { partial } \\
\text { flow of electrons } & \text { pure element } \\
\text { gains } & \text { rarely } \\
\text { half-reactions } & \text { reduced } \\
\text { heat } & \text { reducing } \\
\text { increases } & \text { reducing agent } \\
\text { light } & \text { reduction } \\
\text { loses } & \text { sulfur dioxide } \\
\text { one } & \text { transferred } \\
\text { oxidation } & \text { two or more } \\
\text { oxidized } & \text { water }
\end{array}
$$

In decomposition reactions, _____________ compound is converted into two or more simpler substances.

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Problem 16

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { carbon dioxide } \\
\text { change } & \begin{array}{l}
\text { oxidizing } \\
\text { oxidizing agent }
\end{array} \\
\text { decreases } & \text { partial } \\
\text { flow of electrons } & \text { pure element } \\
\text { gains } & \text { rarely } \\
\text { half-reactions } & \text { reduced } \\
\text { heat } & \text { reducing } \\
\text { increases } & \text { reducing agent } \\
\text { light } & \text { reduction } \\
\text { loses } & \text { sulfur dioxide } \\
\text { one } & \text { transferred } \\
\text { oxidation } & \text { two or more } \\
\text { oxidized } & \text { water }
\end{array}
$$

In a combustion reaction, oxidation is very rapid and is accompanied by _____________ and usually _____________.

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07:37

Problem 17

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { carbon dioxide } \\
\text { change } & \begin{array}{l}
\text { oxidizing } \\
\text { oxidizing agent }
\end{array} \\
\text { decreases } & \text { partial } \\
\text { flow of electrons } & \text { pure element } \\
\text { gains } & \text { rarely } \\
\text { half-reactions } & \text { reduced } \\
\text { heat } & \text { reducing } \\
\text { increases } & \text { reducing agent } \\
\text { light } & \text { reduction } \\
\text { loses } & \text { sulfur dioxide } \\
\text { one } & \text { transferred } \\
\text { oxidation } & \text { two or more } \\
\text { oxidized } & \text { water }
\end{array}
$$

When any substance that contains carbon is combusted (or burned) completely, the carbon forms _____________.

Vishal Sharma
Vishal Sharma
Numerade Educator

Problem 18

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { carbon dioxide } \\
\text { change } & \begin{array}{l}
\text { oxidizing } \\
\text { oxidizing agent }
\end{array} \\
\text { decreases } & \text { partial } \\
\text { flow of electrons } & \text { pure element } \\
\text { gains } & \text { rarely } \\
\text { half-reactions } & \text { reduced } \\
\text { heat } & \text { reducing } \\
\text { increases } & \text { reducing agent } \\
\text { light } & \text { reduction } \\
\text { loses } & \text { sulfur dioxide } \\
\text { one } & \text { transferred } \\
\text { oxidation } & \text { two or more } \\
\text { oxidized } & \text { water }
\end{array}
$$

When a substance that contains hydrogen is burned completely, the hydrogen forms _____________.

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Problem 19

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { carbon dioxide } \\
\text { change } & \begin{array}{l}
\text { oxidizing } \\
\text { oxidizing agent }
\end{array} \\
\text { decreases } & \text { partial } \\
\text { flow of electrons } & \text { pure element } \\
\text { gains } & \text { rarely } \\
\text { half-reactions } & \text { reduced } \\
\text { heat } & \text { reducing } \\
\text { increases } & \text { reducing agent } \\
\text { light } & \text { reduction } \\
\text { loses } & \text { sulfur dioxide } \\
\text { one } & \text { transferred } \\
\text { oxidation } & \text { two or more } \\
\text { oxidized } & \text { water }
\end{array}
$$

When any substance that contains sulfur burns completely, the sulfur forms _____________.

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Problem 20

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { carbon dioxide } \\
\text { change } & \begin{array}{l}
\text { oxidizing } \\
\text { oxidizing agent }
\end{array} \\
\text { decreases } & \text { partial } \\
\text { flow of electrons } & \text { pure element } \\
\text { gains } & \text { rarely } \\
\text { half-reactions } & \text { reduced } \\
\text { heat } & \text { reducing } \\
\text { increases } & \text { reducing agent } \\
\text { light } & \text { reduction } \\
\text { loses } & \text { sulfur dioxide } \\
\text { one } & \text { transferred } \\
\text { oxidation } & \text { two or more } \\
\text { oxidized } & \text { water }
\end{array}
$$

In single‐displacement reactions, atoms of one element in a compound are displaced (or replaced) by atoms from a(n) _____________.

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02:50

Problem 21

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { chemical energy } & \text { not rechargeable } \\
\text { electrical conductors } & \text { oxidation } \\
\text { electrical energy } & \text { positive } \\
\text { electrolysis } & \text { positive electrode } \\
\text { flow } & \text { rechargeable } \\
\text { force } & \text { reduction } \\
\text { half-reactions } & \text { voltaic cells }
\end{array}
$$

Strictly speaking, a battery is a series of _____________ joined in such a way that they work together. A battery can also be described as a device that converts _____________ into _____________ using redox reactions.

Shreestika Pradhan
Shreestika Pradhan
Numerade Educator
02:50

Problem 22

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { chemical energy } & \text { not rechargeable } \\
\text { electrical conductors } & \text { oxidation } \\
\text { electrical energy } & \text { positive } \\
\text { electrolysis } & \text { positive electrode } \\
\text { flow } & \text { rechargeable } \\
\text { force } & \text { reduction } \\
\text { half-reactions } & \text { voltaic cells }
\end{array}
$$

A voltaic cell keeps two oxidation-reduction _____________ separated, causing the electrons released in the oxidation half of the reaction to pass through a wire connecting the two halves of the apparatus.

Shreestika Pradhan
Shreestika Pradhan
Numerade Educator
02:50

Problem 23

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { chemical energy } & \text { not rechargeable } \\
\text { electrical conductors } & \text { oxidation } \\
\text { electrical energy } & \text { positive } \\
\text { electrolysis } & \text { positive electrode } \\
\text { flow } & \text { rechargeable } \\
\text { force } & \text { reduction } \\
\text { half-reactions } & \text { voltaic cells }
\end{array}
$$

Metal strips in voltaic cells are called electrodes, which is the general name for _____________ placed in half‐cells of voltaic cells.

Shreestika Pradhan
Shreestika Pradhan
Numerade Educator
02:50

Problem 24

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { chemical energy } & \text { not rechargeable } \\
\text { electrical conductors } & \text { oxidation } \\
\text { electrical energy } & \text { positive } \\
\text { electrolysis } & \text { positive electrode } \\
\text { flow } & \text { rechargeable } \\
\text { force } & \text { reduction } \\
\text { half-reactions } & \text { voltaic cells }
\end{array}
$$

The electrode at which _____________ occurs in a voltaic cell is called the anode. Because electrons are lost, forming more positive (or less negative) species at the anode, the anode surroundings tend to become more _____________.

Shreestika Pradhan
Shreestika Pradhan
Numerade Educator
02:23

Problem 25

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { chemical energy } & \text { not rechargeable } \\
\text { electrical conductors } & \text { oxidation } \\
\text { electrical energy } & \text { positive } \\
\text { electrolysis } & \text { positive electrode } \\
\text { flow } & \text { rechargeable } \\
\text { force } & \text { reduction } \\
\text { half-reactions } & \text { voltaic cells }
\end{array}
$$

The cathode is the electrode in a voltaic cell at which _____________ occurs. By convention, the cathode is designated the _____________. Because electrons flow along the wire to the cathode, and because substances gain those electrons to become more negative (or less positive), the cathode surroundings tend to become more negative. Thus cations are attracted to the cathode.

ZC
Zhengguo Cai
Numerade Educator
02:50

Problem 26

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { chemical energy } & \text { not rechargeable } \\
\text { electrical conductors } & \text { oxidation } \\
\text { electrical energy } & \text { positive } \\
\text { electrolysis } & \text { positive electrode } \\
\text { flow } & \text { rechargeable } \\
\text { force } & \text { reduction } \\
\text { half-reactions } & \text { voltaic cells }
\end{array}
$$

The component of the voltaic cell through which ions are able to _____________ is called the electrolyte.

Shreestika Pradhan
Shreestika Pradhan
Numerade Educator
02:50

Problem 27

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { chemical energy } & \text { not rechargeable } \\
\text { electrical conductors } & \text { oxidation } \\
\text { electrical energy } & \text { positive } \\
\text { electrolysis } & \text { positive electrode } \\
\text { flow } & \text { rechargeable } \\
\text { force } & \text { reduction } \\
\text { half-reactions } & \text { voltaic cells }
\end{array}
$$

Voltage, a measure of the strength of an electric current, represents the _____________ that moves electrons from the anode to the cathode in a voltaic cell. When a greater voltage is applied in the opposite direction, electrons can be pushed from what would normally be the cathode toward the voltaic cell’s anode. This process is called _____________.

Shreestika Pradhan
Shreestika Pradhan
Numerade Educator

Problem 28

Complete the following statements by writing one of these words or phrases in each blank.
$$
\begin{array}{ll}
\text { chemical energy } & \text { not rechargeable } \\
\text { electrical conductors } & \text { oxidation } \\
\text { electrical energy } & \text { positive } \\
\text { electrolysis } & \text { positive electrode } \\
\text { flow } & \text { rechargeable } \\
\text { force } & \text { reduction } \\
\text { half-reactions } & \text { voltaic cells }
\end{array}
$$

Batteries that are _____________ are called primary batteries. A(n) _____________ battery is called a secondary battery or a storage battery.

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02:40

Problem 29

Describe the difference between the redox reactions that form binary ionic compounds, such as zinc oxide, from their elements and the similar redox reactions that form molecular compounds, such as nitrogen monoxide, from their elements.

David Collins
David Collins
Numerade Educator
01:44

Problem 30

Are the electrons in the following redox reactions transferred completely from the atoms of one element to the atoms of another or are they only partially transferred?
a. $4 \mathrm{Al}(\mathrm{s})+3 \mathrm{O}_2(\mathrm{~g}) \rightarrow 2 \mathrm{Al}_2 \mathrm{O}_3(\mathrm{~s})$
b. $\mathrm{C}(\mathrm{s})+\mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{CO}_2(\mathrm{~g})$

David Collins
David Collins
Numerade Educator
08:11

Problem 31

Are the electrons in the following redox reactions transferred completely from the atoms of one element to the atoms of another or are they only partially transferred?
a. $2 \mathrm{~K}(s)+\mathrm{F}_2(g) \rightarrow 2 \mathrm{KF}(s)$
b. $2 \mathrm{H}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightarrow 2 \mathrm{H}_2 \mathrm{O}(l)$

Emily Wendel
Emily Wendel
Numerade Educator
08:00

Problem 32

Are the electrons in the following redox reactions transferred completely from the atoms of one element to the atoms of another or are they only partially transferred?
a. $\mathrm{S}_8(\mathrm{~s})+8 \mathrm{O}_2(\mathrm{~g}) \rightarrow 8 \mathrm{SO}_2(\mathrm{~g})$
b. $\mathrm{P}_4(s)+6 \mathrm{Cl}_2(g) \rightarrow 4 \mathrm{PCl}_3(l)$

Dr. Satish Ingale
Dr. Satish Ingale
Numerade Educator
04:13

Problem 33

Are the electrons in the following redox reactions transferred completely from the atoms of one element to the atoms of another or are they only partially transferred?
a. $\mathrm{Ca}(s)+\mathrm{Cl}_2(g) \rightarrow \mathrm{CaCl}_2(s)$
b. $4 \mathrm{Cu}(\mathrm{s})+\mathrm{O}_2(\mathrm{~g}) \rightarrow 2 \mathrm{Cu}_2 \mathrm{O}(\mathrm{s})$

Adriano Chikande
Adriano Chikande
Numerade Educator
02:04

Problem 34

Aluminum bromide, $\mathrm{AlBr}_3$, which is used to add bromine atoms to organic compounds, can be made by passing gaseous bromine over hot aluminum. Which of the following half-reactions for this oxidation-reduction reaction describes the oxidation, and which one describes the reduction?

$$
\begin{aligned}
& 2 \mathrm{Al} \rightarrow 2 \mathrm{Al}^{3+}+6 \mathrm{e}^{-} \\
& 3 \mathrm{Br}_2+6 \mathrm{e}^{-} \rightarrow 6 \mathrm{Br}^{-}
\end{aligned}
$$

Carolina Acevedo
Carolina Acevedo
Numerade Educator
06:39

Problem 35

Iodine, $\mathrm{I}_2$, has many uses, including the production of dyes, antiseptics, photographic film, pharmaceuticals, and medicinal soaps. It forms when chlorine, $\mathrm{Cl}_2$, reacts with iodide ions in a sodium iodide solution. Which of the following half-reactions for this oxidation-reduction reaction describes the oxidation, and which one describes the reduction?

$$
\begin{aligned}
& \mathrm{Cl}_2+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{Cl}^{-} \\
& 2 \mathrm{I}^{-} \rightarrow \mathrm{I}_2+2 \mathrm{e}^{-}
\end{aligned}
$$

Nicole Chung
Nicole Chung
Numerade Educator
01:58

Problem 36

Determine the oxidation number for the atoms of each element in the following formulas.
a. $\mathrm{S}_8$
c. $\mathrm{Na}_2 \mathrm{~S}$
b. $S^{2-}$
d. FeS

David Collins
David Collins
Numerade Educator
05:45

Problem 37

Determine the oxidation number for the atoms of each element in the following formulas.
a. $\mathrm{P}_4$
d. $\mathrm{P}_2 \mathrm{O}_3$
b. $\mathrm{PF}_3$
e. $\mathrm{H}_3 \mathrm{PO}_4$
c. $\mathrm{PH}_3$

Emily Wendel
Emily Wendel
Numerade Educator
03:02

Problem 38

Determine the oxidation number for the atoms of each element in the following formulas.
a. $\mathrm{Sc}_2 \mathrm{O}_3$
c. $\mathrm{N}_2$
b. RbH
d. $\mathrm{NH}_3$

Emily Wendel
Emily Wendel
Numerade Educator
01:52

Problem 39

Determine the oxidation number for the atoms of each element in the following formulas.
a. $\mathrm{N}^{3-}$
c. $\mathrm{K}_3 \mathrm{~N}$
b. $\mathrm{N}_2 \mathrm{O}_5$

Eileen Sullivan
Eileen Sullivan
Numerade Educator
03:49

Problem 40

Determine the oxidation number for the atoms of each element in the following formulas.
a. $\mathrm{ClF}_3$
c. $\mathrm{H}_2 \mathrm{SO}_4$
b. $\mathrm{H}_2 \mathrm{O}_2$

Emily Wendel
Emily Wendel
Numerade Educator
01:25

Problem 41

Determine the oxidation number for the atoms of each element in the following formulas.
a. $\mathrm{Co}_3 \mathrm{~N}_2$
c. NaH
b. Na

Susan Hallstrom
Susan Hallstrom
Numerade Educator
05:46

Problem 42

Determine the oxidation number for the atoms of each element in the following formulas.
a. $\mathrm{HPO}_4{ }^{2-}$
c. $\mathrm{N}_2 \mathrm{O}_4{ }^{2-}$
b. $\mathrm{NiSO}_4$
d. $\mathrm{Mn}_3\left(\mathrm{PO}_4\right)_2$

Emily Wendel
Emily Wendel
Numerade Educator
05:46

Problem 43

Determine the oxidation number for the atoms of each element in the following formulas.
a. $\mathrm{HSO}_3^{-}$
c. $\mathrm{Cu}_3\left(\mathrm{PO}_4\right)_2$
b. $\mathrm{Cu}\left(\mathrm{NO}_3\right)_2$

Emily Wendel
Emily Wendel
Numerade Educator
01:40

Problem 44

The following partial reactions represent various means by which bacteria obtain energy. Determine the oxidation number for each atom other than oxygen and hydrogen atoms, and decide whether the half-reaction represents oxidation or reduction. None of the oxygen or hydrogen atoms are oxidized or reduced.

$$
\begin{aligned}
& 2 \mathrm{Fe}^{2+} \rightarrow \mathrm{Fe}_2 \mathrm{O}_3+\text { energy } \\
& 2 \mathrm{NH}_3 \rightarrow 2 \mathrm{NO}_2^{-}+3 \mathrm{H}_2 \mathrm{O}+\text { energy } \\
& 2 \mathrm{NO}_2^{-}+\mathrm{O}_2 \rightarrow 2 \mathrm{NO}_3^{-}+\text {energy } \\
& 8 \mathrm{H}_2 \mathrm{~S} \rightarrow \mathrm{~S}_8+8 \mathrm{H}_2 \mathrm{O}+\text { energy } \\
& \mathrm{S}_8+8 \mathrm{H}_2 \mathrm{O} \rightarrow \mathrm{SO}_4^{2-}+16 \mathrm{H}^{+}+\text {energy }
\end{aligned}
$$

Nicole Krahulik
Nicole Krahulik
Numerade Educator
08:14

Problem 45

About $47 \%$ of the hydrochloric acid produced in the U.S. is used for cleaning metallic surfaces. Hydrogen chloride, HCl , which is dissolved in water to make the acid, is formed in the reaction of chlorine gas and hydrogen gas, displayed below. Determine the oxidation number for each atom in the equation, and decide whether the reaction is a redox reaction or not. If it is redox, identify which substance is oxidized, which substance is reduced, the oxidizing agent, and the reducing agent.

$$
\mathrm{Cl}_2(\mathrm{~g})+\mathrm{H}_2(\mathrm{~g}) \rightarrow 2 \mathrm{HCl}(\mathrm{~g})
$$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
07:06

Problem 46

The following equation describes the reaction that produces hydrofluoric acid, which is used to make chlorofluorocarbons (CFCs). Determine the oxidation number for each atom in the equation, and decide whether the reaction is a redox reaction or not. If it is redox, identify which substance is oxidized, which substance is reduced, the oxidizing agent, and the reducing agent.

$$
\mathrm{CaF}_2+\mathrm{H}_2 \mathrm{SO}_4 \rightarrow 2 \mathrm{HF}+\mathrm{CaSO}_4
$$

Christopher Nilsen
Christopher Nilsen
Numerade Educator
01:21

Problem 47

Water and carbon dioxide fire extinguishers should not be used on magnesium fires because both substances react with magnesium and generate enough heat to intensify the fire. Determine the oxidation number for each atom in the equations that describe these reactions (displayed below), and decide whether each reaction is a redox reaction or not. If it is redox, identify which substance is oxidized, which substance is reduced, the oxidizing agent, and the reducing agent.

$$
\begin{aligned}
\mathrm{Mg}(s)+2 \mathrm{H}_2 \mathrm{O}(l) & \rightarrow \mathrm{Mg}(\mathrm{OH})_2(a q)+\mathrm{H}_2(g)+\text { heat } \\
2 \mathrm{Mg}(s)+\mathrm{CO}_2(g) & \rightarrow 2 \mathrm{MgO}(s)+\mathrm{C}(s)+\text { heat }
\end{aligned}
$$

Lottie Adams
Lottie Adams
Numerade Educator
02:40

Problem 48

Potassium nitrate is used in the production of fireworks, explosives, and matches. It is also used in curing foods and to modify the burning properties of tobacco. The reaction for the industrial production of $\mathrm{KNO}_3$ is summarized below. Determine the oxidation number for each atom, and decide whether the reaction is a redox reaction or not. If it is redox, identify which substance is oxidized, which substance is reduced, the oxidizing agent, and the reducing agent.

$$
4 \mathrm{KCl}+4 \mathrm{HNO}_3+\mathrm{O}_2 \rightarrow 4 \mathrm{KNO}_3+2 \mathrm{Cl}_2+2 \mathrm{H}_2 \mathrm{O}
$$

David Collins
David Collins
Numerade Educator
00:53

Problem 49

Formaldehyde, $\mathrm{CH}_2 \mathrm{O}$, which is used in embalming fluids, is made from methanol in the reaction described below. Determine the oxidation number for each atom in this equation, and decide whether the reaction is a redox reaction or not. If it is redox, identify which substance is oxidized, which substance is reduced, the oxidizing agent, and the reducing agent.

$$
2 \mathrm{CH}_3 \mathrm{OH}+\mathrm{O}_2 \rightarrow 2 \mathrm{CH}_2 \mathrm{O}+2 \mathrm{H}_2 \mathrm{O}
$$

David Collins
David Collins
Numerade Educator
00:52

Problem 50

The weak acid hydrofluoric acid, $\operatorname{HF}(\mathrm{aq})$, is used to frost light bulbs. It reacts with the silicon dioxide in glass on the inside of light bulbs to form a white substance, $\mathrm{H}_2 \mathrm{SiF}_6$, that deposits on the glass and reduces the glare from the bulb. The same reaction is run on a larger scale to produce $\mathrm{H}_2 \mathrm{SiF}_6$ used for fluoridating drinking water. Determine the oxidation number for each atom in the reaction, and decide whether the reaction is a redox reaction or not. If it is redox, identify which substance is oxidized, which substance is reduced, the oxidizing agent, and the reducing agent.

$$
6 \mathrm{HF}+\mathrm{SiO}_2 \rightarrow \mathrm{H}_2 \mathrm{SiF}_6+2 \mathrm{H}_2 \mathrm{O}
$$

Ronald Prasad
Ronald Prasad
Numerade Educator
06:41

Problem 51

For each of the following equations, determine the oxidation number for each atom in the equation and identify whether the reaction is a redox reaction or not. If the reaction is redox, identify what is oxidized, what is reduced, the oxidizing agent, and the reducing agent.
a. $\mathrm{Co}(s)+2 \mathrm{AgNO}_3(a q) \rightarrow \mathrm{Co}\left(\mathrm{NO}_3\right)_2(a q)+2 \mathrm{Ag}(s)$
b. $\mathrm{V}_2 \mathrm{O}_5(s)+5 \mathrm{Ca}(l) \xrightarrow{\Delta} 2 \mathrm{~V}(l)+5 \mathrm{CaO}(s)$
c. $\mathrm{CaCO}_3(\mathrm{aq})+\mathrm{SiO}_2(\mathrm{~s}) \rightarrow \mathrm{CaSiO}_3(\mathrm{~s})+\mathrm{CO}_2(\mathrm{~g})$
d. $2 \mathrm{NaH}(\mathrm{s}) \xrightarrow{\Delta} 2 \mathrm{Na}(\mathrm{s})+\mathrm{H}_2(\mathrm{~g})$
e. $5 \mathrm{As}_4 \mathrm{O}_6(s)+8 \mathrm{KMnO}_4(a q)+18 \mathrm{H}_2 \mathrm{O}(l)+52 \mathrm{KCl}(a q) \rightarrow 20 \mathrm{~K}_3 \mathrm{AsO}_4(a q)+8 \mathrm{MnCl}_2(a q)+36 \mathrm{HCl}(a q)$

David Collins
David Collins
Numerade Educator
13:03

Problem 52

For each of the following equations, determine the oxidation number for each atom in the equation and identify whether the reaction is a redox reaction or not. If the reaction is redox, identify what is oxidized, what is reduced, the oxidizing agent, and the reducing agent.
a. $2 \mathrm{Na}(s)+2 \mathrm{H}_2 \mathrm{O}(l) \rightarrow 2 \mathrm{NaOH}(a q)+\mathrm{H}_2(g)$
b. $\mathrm{HCl}(\mathrm{aq})+\mathrm{NH}_3(\mathrm{aq}) \rightarrow \mathrm{NH}_4 \mathrm{Cl}(a q)$
c. $2 \mathrm{Cr}(s)+3 \mathrm{CuSO}_4(a q) \rightarrow \mathrm{Cr}_2\left(\mathrm{SO}_4\right)_3(a q)+3 \mathrm{Cu}(s)$
d. $3 \mathrm{H}_2 \mathrm{SO}_3(\mathrm{aq})+2 \mathrm{HNO}_3(\mathrm{aq}) \rightarrow 2 \mathrm{NO}(\mathrm{g})+\mathrm{H}_2 \mathrm{O}(l)+3 \mathrm{H}_2 \mathrm{SO}_4(\mathrm{aq})$
e. $\mathrm{CaO}(s)+\mathrm{H}_2 \mathrm{O}(l) \rightarrow \mathrm{Ca}^{2+}(a q)+2 \mathrm{OH}^{-}(a q)$

Shahina -
Shahina -
Numerade Educator
07:58

Problem 53

The following equations summarize the steps in the process used to make most of the sulfuric acid produced in the United States. Determine the oxidation number for each atom in each of the following equations, and identify whether each reaction is a redox reaction or not. For the redox reactions, identify what is oxidized, what is reduced, the oxidizing agent, and the reducing agent.

$$
\begin{aligned}
& 1 / 8 \mathrm{~S}_8+\mathrm{O}_2 \rightarrow \mathrm{SO}_2 \\
& \mathrm{SO}_2+1 / 2 \mathrm{O}_2 \rightarrow \mathrm{SO}_3 \\
& \mathrm{SO}_3+\mathrm{H}_2 \mathrm{O} \rightarrow \mathrm{H}_2 \mathrm{SO}_4
\end{aligned}
$$

Vishal Sharma
Vishal Sharma
Numerade Educator
06:50

Problem 54

Because of its superior hiding ability, titanium dioxide has been the best selling white pigment since 1939. In 1990, there were 2.16 billion pounds of it sold in the United States for a variety of purposes, including surface coatings (paint), plastics, and paper. The following equations show how impure $\mathrm{TiO}_2$ is purified. Determine the oxidation number for each atom in them and identify whether each reaction is a redox reaction or not. For the redox reactions, identify what is oxidized, what is reduced, the oxidizing agent, and the reducing agent.

$$
\begin{aligned}
& 3 \mathrm{TiO}_2+4 \mathrm{C}+6 \mathrm{Cl}_2 \rightarrow 3 \mathrm{TiCl}_4+2 \mathrm{CO}+2 \mathrm{CO}_2 \\
& \mathrm{TiCl}_4+\mathrm{O}_2 \rightarrow \mathrm{TiO}_2+2 \mathrm{Cl}_2
\end{aligned}
$$

Cameron Oden
Cameron Oden
Numerade Educator
02:38

Problem 55

Classify each of these reactions with respect to the following categories: combination reaction, decomposition reaction, combustion reaction, and single-displacement reaction.
a. $2 \mathrm{NaH}(s) \rightarrow 2 \mathrm{Na}(s)+\mathrm{H}_2(g)$
b. $2 \mathrm{KI}(a q)+\mathrm{Cl}_2(g) \rightarrow 2 \mathrm{KCl}(a q)+\mathrm{I}_2(s)$
c. $2 \mathrm{C}_2 \mathrm{H}_5 \mathrm{SH}(l)+9 \mathrm{O}_2(g) \rightarrow 4 \mathrm{CO}_2(g)+6 \mathrm{H}_2 \mathrm{O}(l)+2 \mathrm{SO}_2(g)$
d. $\mathrm{H}_2(\mathrm{~g})+\mathrm{CuO}(\mathrm{s}) \xrightarrow{\Delta} \mathrm{Cu}(\mathrm{s})+\mathrm{H}_2 \mathrm{O}(l)$
e. $\mathrm{P}_4(\mathrm{~s})+5 \mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{P}_4 \mathrm{O}_{10}(\mathrm{~s})$

Emily Himsel
Emily Himsel
Numerade Educator
02:42

Problem 56

Classify each of these reactions with respect to the following categories: combination reaction, decomposition reaction, combustion reaction, and single-displacement reaction.
a. $\mathrm{Fe}_2\left(\mathrm{CO}_3\right)_2(s) \xrightarrow{\Delta} \mathrm{Fe}_2 \mathrm{O}_3(s)+2 \mathrm{CO}_2(g)$
b. $2 \mathrm{C}_6 \mathrm{H}_{11} \mathrm{OH}(l)+17 \mathrm{O}_2(g) \rightarrow 12 \mathrm{CO}_2(g)+12 \mathrm{H}_2 \mathrm{O}(l)$
c. $\mathrm{P}_4 \mathrm{O}_{10}(s)+6 \mathrm{H}_2 \mathrm{O}(l) \rightarrow 4 \mathrm{H}_3 \mathrm{PO}_4(a q)$
d. $2 \mathrm{C}(\mathrm{s})+\mathrm{MnO}_2(\mathrm{~s}) \xrightarrow{\Delta} \mathrm{Mn}(\mathrm{s})+2 \mathrm{CO}(\mathrm{g})$
e. $2 \mathrm{NaClO}_3(\mathrm{~s}) \xrightarrow{\Delta} 2 \mathrm{NaCl}(\mathrm{s})+3 \mathrm{O}_2(\mathrm{~g})$

Emily Himsel
Emily Himsel
Numerade Educator
02:42

Problem 57

Classify each of these reactions with respect to the following categories: combination reaction, decomposition reaction, combustion reaction, and single-displacement reaction.
a. $4 \mathrm{~B}(\mathrm{~s})+3 \mathrm{O}_2(\mathrm{~g}) \rightarrow 2 \mathrm{~B}_2 \mathrm{O}_3(\mathrm{~s})$
b. $\left(\mathrm{C}_2 \mathrm{H}_5\right)_2 \mathrm{O}(l)+6 \mathrm{O}_2(g) \rightarrow 4 \mathrm{CO}_2(g)+5 \mathrm{H}_2 \mathrm{O}(l)$
c. $2 \mathrm{Cr}_2 \mathrm{O}_3(s)+3 \mathrm{Si}(s) \xrightarrow{\Delta} 4 \mathrm{Cr}(s)+3 \mathrm{SiO}_2(s)$
d. $\mathrm{C}_6 \mathrm{H}_{11} \mathrm{SH}(l)+10 \mathrm{O}_2(\mathrm{~g}) \rightarrow 6 \mathrm{CO}_2(g)+6 \mathrm{H}_2 \mathrm{O}(l)+\mathrm{SO}_2(g)$
e. $2 \mathrm{NaHCO}_3(s) \xrightarrow{\Delta} \mathrm{Na}_2 \mathrm{CO}_3(s)+\mathrm{H}_2 \mathrm{O}(l)+\mathrm{CO}_2(g)$

Emily Himsel
Emily Himsel
Numerade Educator
02:38

Problem 58

Classify each of these reactions with respect to the following categories: combination reaction, decomposition reaction, combustion reaction, and single-displacement reaction.
a. $3 \mathrm{H}_2(\mathrm{~g})+\mathrm{WO}_3(\mathrm{~s}) \xrightarrow{\Delta} \mathrm{W}(\mathrm{s})+3 \mathrm{H}_2 \mathrm{O}(l)$
b. $2 \mathrm{I}_4 \mathrm{O}_9(s) \rightarrow 2 \mathrm{I}_2 \mathrm{O}_6(s)+2 \mathrm{I}_2(s)+3 \mathrm{O}_2(g)$
c. $2 \mathrm{NaNO}_3(\mathrm{~s}) \xrightarrow{\Delta} 2 \mathrm{NaNO}_2(\mathrm{~s})+\mathrm{O}_2(\mathrm{~g})$
d. $\mathrm{Cl}_2(g)+2 \mathrm{KBr}(a q) \rightarrow 2 \mathrm{KCl}(a q)+\mathrm{Br}_2(l)$

Emily Himsel
Emily Himsel
Numerade Educator
06:08

Problem 59

Write balanced equations for the complete combustion of each of the following substances.
a. $\mathrm{C}_3 \mathrm{H}_8(\mathrm{~g})$
b. $\mathrm{C}_4 \mathrm{H}_9 \mathrm{OH}(l)$
c. $\mathrm{CH}_3 \mathrm{COSH}(l)$

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:55

Problem 60

Write balanced equations for the complete combustion of each of the following substances.
a. $\mathrm{C}_{13} \mathrm{H}_{28}(l)$
b. $\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}(s)$
c. $\mathrm{C}_2 \mathrm{H}_5 \mathrm{SO}_3 \mathrm{H}(l)$

Rithvik Manne
Rithvik Manne
Numerade Educator
View

Problem 61

The following pairs react in single-displacement reactions that are similar to the reaction between uncharged zinc metal and the copper(II) ions in a copper(II) sulfate solution. Describe the changes in these reactions, including the nature of the particles in the system before the reaction takes place, the nature of the reaction itself, and the nature of the particles in the system after the reaction. Your description should also include the equations for the half-reactions and the net ionic equation for the overall reaction.
a. Magnesium metal and nickel(II) nitrate, $\mathrm{Ni}\left(\mathrm{NO}_3\right)_2(a q)$
b. Calcium metal and cobalt(II) chloride, $\mathrm{CoCl}_2(\mathrm{aq})$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
01:40

Problem 62

We know that the following reaction can by used to generate an electric current in a voltaic cell.

$$
\mathrm{Zn}(s)+\mathrm{CuSO}_4(a q) \rightarrow \mathrm{Cu}(s)+\mathrm{ZnSO}_4(a q)
$$

Sketch similar voltaic cells made from each of the reactions presented below, showing the key components of the two half-cells and indicating the cathode electrode and the anode electrode, the negative and positive electrodes, the direction of movement of the electrons in the wire between the electrodes, and the direction of movement of the ions in the system. Show a salt bridge in each sketch, and show the movement of ions out of the salt bridge.
a. $\mathrm{Mn}(s)+\mathrm{PbCl}_2(a q) \rightarrow \mathrm{Pb}(s)+\mathrm{MnCl}_2(a q)$
b. $\mathrm{Mg}(s)+2 \mathrm{AgNO}_3(a q) \rightarrow 2 \mathrm{Ag}(s)+\mathrm{Mg}\left(\mathrm{NO}_3\right)_2(a q)$

Lottie Adams
Lottie Adams
Numerade Educator
02:11

Problem 63

The following equation summarizes the chemical changes that take place in a typical dry cell.

$$
\begin{aligned}
& \mathrm{Zn}(s)+2 \mathrm{MnO}_2(s)+2 \mathrm{NH}_4^{+}(a q) \\
& \rightarrow \mathrm{Zn}^{2+}(a q)+\mathrm{Mn}_2 \mathrm{O}_3(s)+2 \mathrm{NH}_3(a q)+\mathrm{H}_2 \mathrm{O}(l)
\end{aligned}
$$

Determine the oxidation number for each atom in the equation, and identify what is oxidized, what is reduced, the oxidizing agent, and the reducing agent.

Nicole Mabante
Nicole Mabante
Numerade Educator
00:53

Problem 64

The following equation summarizes the chemical changes that take place in a nickel-cadmium battery. Determine the oxidation number for each atom in the equation, and identify what is oxidized, what is reduced, the oxidizing agent, and the reducing agent.

$$
\mathrm{Cd}(s)+2 \mathrm{NiO}(\mathrm{OH})(s)+2 \mathrm{H}_2 \mathrm{O}(l) \rightarrow \mathrm{Cd}(\mathrm{OH})_2(s)+2 \mathrm{Ni}(\mathrm{OH})_2(s)
$$

David Collins
David Collins
Numerade Educator
03:25

Problem 65

The following equation summarizes the chemical changes that take place in a lead-acid battery. Determine the oxidation number for each atom in the equation, and identify what is oxidized, what is reduced, the oxidizing agent, and the reducing agent.

$$
\mathrm{Pb}(s)+\mathrm{PbO}_2(s)+2 \mathrm{HSO}_4^{-}(a q)+2 \mathrm{H}_3 \mathrm{O}^{+}(a q) \rightarrow 2 \mathrm{PbSO}_4(s)+4 \mathrm{H}_2 \mathrm{O}(l)
$$

Susan Hallstrom
Susan Hallstrom
Numerade Educator
03:19

Problem 66

Nitric acid, which is used to produce fertilizers and explosives, is made in the following three steps. Determine the oxidation number for each atom in the three equations and identify whether each reaction is a redox reaction or not. If a reaction is redox, identify what is oxidized and what is reduced.

$$
\begin{aligned}
& 4 \mathrm{NH}_3+5 \mathrm{O}_2 \rightarrow 4 \mathrm{NO}+6 \mathrm{H}_2 \mathrm{O} \\
& 2 \mathrm{NO}^2+\mathrm{O}_2 \rightarrow 2 \mathrm{NO}_2 \\
& 3 \mathrm{NO}_2+\mathrm{H}_2 \mathrm{O} \rightarrow 2 \mathrm{HNO}_3+\mathrm{NO}
\end{aligned}
$$

Lottie Adams
Lottie Adams
Numerade Educator
View

Problem 67

Sodium hydrogen carbonate, $\mathrm{NaHCO}_3$, best known as the active ingredient in baking soda, is used in several ways in food preparation. It is also added to animal feeds and used to make soaps and detergents. Baking soda can also be used to put out small fires on your stovetop. The heat of the flames causes the $\mathrm{NaHCO}_3$ to decompose to form carbon dioxide, which displaces the air above the flames depriving the fire of the oxygen necessary for combustion. The equation for the reaction is below.

$$
2 \mathrm{NaHCO}_3(s) \xrightarrow{\Delta} \mathrm{Na}_2 \mathrm{CO}_3(s)+\mathrm{H}_2 \mathrm{O}(l)+\mathrm{CO}_2(g)
$$

Determine the oxidation number for each atom in the equation and identify whether the reaction is a redox reaction or not. If the reaction is redox, identify what is oxidized and what is reduced.

Bridger Johnston
Bridger Johnston
Numerade Educator
02:28

Problem 68

Swimming pools can be chlorinated by adding either calcium hypochlorite, $\mathrm{Ca}(\mathrm{OCl})_2$, or sodium hypochlorite, NaOCl . The active component is the hypochlorite ion, $\mathrm{OCl}^{-}$. Because the rate of the following reaction is increased by ultraviolet radiation in sunlight, it is best to chlorinate pools in the evening to avoid the hypochlorite ion's decomposition.

$$
\mathrm{OCl}^{-}(a q) \rightarrow \mathrm{Cl}^{-}(a q)+1 / 2 \mathrm{O}_2(g)
$$

Determine the oxidation number for each atom in the equation and identify whether the reaction is a redox reaction or not. If the reaction is redox, identify what is oxidized and what is reduced.

Crystal Wang
Crystal Wang
Numerade Educator
04:00

Problem 69

In the past, mercury batteries were commonly used to power electronic watches and small appliances. The overall reaction for this type of battery is

$$
\mathrm{HgO}(s)+\mathrm{Zn}(s) \rightarrow \mathrm{ZnO}(s)+\mathrm{Hg}(l)
$$

Determine the oxidation number for each atom in the equation and decide whether the reaction is a redox reaction or not. If it is redox, identify which substance is oxidized, which substance is reduced, the oxidizing agent, and the reducing agent.

Shubham Kumar
Shubham Kumar
Numerade Educator
01:17

Problem 70

Silver batteries have been used to run heart pacemakers and hearing aids. The overall reaction for this type of battery is

$$
\mathrm{Ag}_2 \mathrm{O}(s)+\mathrm{Zn}(s) \rightarrow \mathrm{ZnO}(s)+2 \mathrm{Ag}(s)
$$

Determine the oxidation number for each atom in the equation and decide whether the reaction is a redox reaction or not. If it is redox, identify which substance is oxidized, which substance is reduced, the oxidizing agent, and the reducing agent.

David Collins
David Collins
Numerade Educator
01:11

Problem 71

$\mathrm{Mn}_3\left(\mathrm{PO}_4\right)_2$, which is used to make corrosion resistant coatings on steel, aluminum, and other metals, is made from the reaction of $\mathrm{Mn}(\mathrm{OH})_2$ with $\mathrm{H}_3 \mathrm{PO}_4$.

$$
3 \mathrm{Mn}(\mathrm{OH})_2(s)+2 \mathrm{H}_3 \mathrm{PO}_4(a q) \rightarrow \mathrm{Mn}_3\left(\mathrm{PO}_4\right)_2(s)+6 \mathrm{H}_2 \mathrm{O}(l)
$$

Determine the oxidation number for each atom in the equation and identify whether the reaction is a redox reaction or not. If it is redox, identify what is oxidized, what is reduced, the oxidizing agent, and the reducing agent.

David Collins
David Collins
Numerade Educator
08:50

Problem 72

One of the ways that plants generate oxygen is represented by the following reaction.

$$
2 \mathrm{Mn}^{4+}+2 \mathrm{H}_2 \mathrm{O} \rightarrow 2 \mathrm{Mn}^{2+}+4 \mathrm{H}^{+}+\mathrm{O}_2
$$

Determine the oxidation number for each atom in the equation and decide whether the reaction is a redox reaction or not. If it is redox, identify which substance is oxidized, which substance is reduced, the oxidizing agent, and the reducing agent.

Vishal Sharma
Vishal Sharma
Numerade Educator
02:51

Problem 73

The noble gases in group 18 on the periodic table used to be called the inert gases because they were thought to be incapable of forming compounds. Their name has been changed to noble gases because although they resist combining with the more common elements to their left on the periodic table, they do mingle with them on rare occasions. The following equations describe reactions that form xenon compounds. Determine the oxidation number for each atom in the reactions, and identify each reaction as redox or not. If it is redox, identify which substance is oxidized, which substance is reduced, the oxidizing agent, and the reducing agent.

$$
\begin{aligned}
& \mathrm{Xe}+3 \mathrm{~F}_2 \rightarrow \mathrm{XeF}_6 \\
& \mathrm{XeF}_6+\mathrm{H}_2 \mathrm{O} \rightarrow \mathrm{XeOF}_4+2 \mathrm{HF} \\
& \mathrm{XeF}_6+\mathrm{OPF}_3 \rightarrow \mathrm{XeOF}_4+\mathrm{PF}_5
\end{aligned}
$$

Nadia Lara
Nadia Lara
Numerade Educator
11:45

Problem 74

Sometimes one of the elements in a reactant appears in more than one product of a reaction and has in one product, a higher oxidation number than before the reaction and in the other product, a lower oxidation number than before the reaction. In this way, the same element is both oxidized and reduced, and the same compound is both the oxidizing agent and the reducing agent. This process is called disproportionation. For example, iodine monofluoride, IF, disproportionates into iodine and iodine pentafluoride in the following reaction:

$$
5 \mathrm{IF} \rightarrow 2 \mathrm{I}_2+\mathrm{IF}_5
$$

Determine the oxidation number for each atom in this equation and show that iodine is both oxidized and reduced and that iodine monofluoride is both the oxidizing agent and the reducing agent.

Jennifer Landry
Jennifer Landry
Numerade Educator
01:41

Problem 75

Sodium perbromate is an oxidizing agent that can be made in the two ways represented by the equations below. The first equation shows the way it was made in the past, and the second equation represents the technique used today.

$$
\begin{aligned}
& \mathrm{NaBrO}_3+\mathrm{XeF}_2+\mathrm{H}_2 \mathrm{O} \rightarrow \mathrm{NaBrO}_4+2 \mathrm{HF}+\mathrm{Xe} \\
& \mathrm{NaBrO}_3+\mathrm{F}_2+2 \mathrm{NaOH} \rightarrow \mathrm{NaBrO}_4+2 \mathrm{NaF}+\mathrm{H}_2 \mathrm{O}
\end{aligned}
$$

Determine the oxidation number for each atom in each of these equations, and decide whether each reaction is a redox reaction or not. If a reaction is a redox reaction, identify which substance is oxidized, which substance is reduced, the oxidizing agent, and the reducing agent.

David Collins
David Collins
Numerade Educator
04:12

Problem 76

Calcium hydrogen sulfite, $\mathrm{Ca}\left(\mathrm{HSO}_3\right)_2$, which is used as a paper pulp preservative and as a disinfectant, is made by reacting sulfur dioxide with calcium hydroxide.

$$
2 \mathrm{SO}_2+\mathrm{Ca}(\mathrm{OH})_2 \rightarrow \mathrm{Ca}\left(\mathrm{HSO}_3\right)_2
$$

Determine the oxidation number for each atom in the equation and decide whether the reaction is a redox reaction or not. If the reaction is a redox reaction, identify which substance is oxidized, which substance is reduced, the oxidizing agent, and the reducing agent.

Allison Krajewski
Allison Krajewski
Numerade Educator
02:31

Problem 77

The following equations represent reactions that involve only halogen atoms. Iodine pentafluoride, $\mathrm{IF}_5$, is used to add fluorine atoms to other compounds, bromine pentafluoride, $\mathrm{BrF}_5$, is an oxidizing agent in liquid rocket propellants, and chlorine trifluoride, $\mathrm{ClF}_3$, is used to reprocess nuclear reactor fuels.

$$
\begin{aligned}
& \mathrm{IF}(g)+2 \mathrm{~F}_2(g) \rightarrow \mathrm{IF}_5 \\
& \mathrm{BrF}(g)+2 \mathrm{~F}_2(g) \rightarrow \mathrm{BrF}_5(g) \\
& \mathrm{Cl}_2(g)+3 \mathrm{~F}_2(g) \rightarrow 2 \mathrm{ClF}_3(g)
\end{aligned}
$$

Determine the oxidation number for each atom in these equations, and decide whether each reaction is a redox reaction or not. If a reaction is a redox reaction, identify which substance is oxidized, which substance is reduced, the oxidizing agent, and the reducing agent.

Lottie Adams
Lottie Adams
Numerade Educator
04:07

Problem 78

The water solution of hydrogen peroxide, $\mathrm{H}_2 \mathrm{O}_2$, used as an antiseptic (3\%) and bleach ( $6 \%$ ) are stored in dark plastic bottles because the reaction below is accelerated by the metal ions found in glass and by light.

$$
2 \mathrm{H}_2 \mathrm{O}_2(\mathrm{aq}) \rightarrow 2 \mathrm{H}_2 \mathrm{O}(l)+\mathrm{O}_2(\mathrm{~g})
$$

Determine the oxidation number for each atom in the equation and identify whether the reaction is a redox reaction or not. If the reaction is redox, identify what is oxidized and what is reduced.

Ronald Prasad
Ronald Prasad
Numerade Educator
02:30

Problem 79

Sodium sulfate, which is used to make detergents and glass, is formed in the following reaction.

$$
4 \mathrm{NaCl}+2 \mathrm{SO}_2+2 \mathrm{H}_2 \mathrm{O}+\mathrm{O}_2 \rightarrow 2 \mathrm{Na}_2 \mathrm{SO}_4+4 \mathrm{HCl}
$$

Determine the oxidation number for each atom in the equation and decide whether the reaction is a redox reaction or not. If a reaction is a redox reaction, identify which substance is oxidized, which substance is reduced, the oxidizing agent, and the reducing agent.

Shazia Naz
Shazia Naz
Numerade Educator
05:35

Problem 80

Hydrogen gas can be made in two steps:

$$
\begin{aligned}
& \mathrm{CH}_4(\mathrm{~g})+\mathrm{H}_2 \mathrm{O}(\mathrm{~g}) \rightarrow \mathrm{CO}(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \\
& \mathrm{CO}(\mathrm{~g})+\mathrm{H}_2 \mathrm{O}(\mathrm{~g}) \rightarrow \mathrm{CO}_2(\mathrm{~g})+\mathrm{H}_2(\mathrm{~g})
\end{aligned}
$$

Determine the oxidation number for each atom in these equations and decide whether each reaction is a redox reaction or not. If a reaction is redox, identify which substance is oxidized and which substance is reduced. (You do not need to identify the oxidizing agent and the reducing agent.)

David Collins
David Collins
Numerade Educator
04:04

Problem 81

Elemental sulfur is produced by the chemical industry from naturally occurring hydrogen sulfide in the following steps.

$$
\begin{aligned}
& 2 \mathrm{H}_2 \mathrm{~S}+3 \mathrm{O}_2 \rightarrow 2 \mathrm{SO}_2+2 \mathrm{H}_2 \mathrm{O} \\
& \mathrm{SO}_2+2 \mathrm{H}_2 \mathrm{~S} \rightarrow 3 \mathrm{~S}+2 \mathrm{H}_2 \mathrm{O}
\end{aligned}
$$

Determine the oxidation number for each atom in these equations and decide whether each reaction is a redox reaction or not. If a reaction is a redox reaction, identify which substance is oxidized, which substance is reduced, the oxidizing agent, and the reducing agent.

Sam Limsuwannarot
Sam Limsuwannarot
Numerade Educator
02:28

Problem 82

Sodium chlorate, $\mathrm{NaClO}_3$, which is used to bleach paper, is made in the following reactions. Determine the oxidation number for each atom in the equations and identify whether each reaction is a redox reaction or not. If a reaction is redox, identify what is oxidized and what is reduced.

$$
\begin{aligned}
& \mathrm{Cl}_2+2 \mathrm{NaOH} \rightarrow \mathrm{NaOCl}+\mathrm{NaCl}+\mathrm{H}_2 \mathrm{O} \\
& 3 \mathrm{NaOCl} \rightarrow \mathrm{NaClO}_3+2 \mathrm{NaCl}
\end{aligned}
$$

Crystal Wang
Crystal Wang
Numerade Educator
09:18

Problem 83

Leaded gasoline, originally developed to decrease pollution, is now banned because the lead(II) bromide, $\mathrm{PbBr}_2$, emitted when it burns decomposes in the atmosphere into two serious pollutants, lead and bromine. The equation for this reaction is below. Determine the oxidation number for each atom in the equation and identify whether the reaction is a redox reaction or not. If the reaction is redox, identify what is oxidized and what is reduced.

$$
\mathrm{PbBr}_2 \xrightarrow{\text { sunlight }} \mathrm{Pb}+\mathrm{Br}_2
$$

Vishal Sharma
Vishal Sharma
Numerade Educator
16:31

Problem 84

When leaded gasoline was banned, there was a rush to find safer ways to reduce emissions of unburned hydrocarbons from gasoline engines. One alternative is to add methyl t-butyl ether (MTBE). In 1990, about 25\% of the methanol, $\mathrm{CH}_3 \mathrm{OH}$, produced by the U.S. chemical industry was used to make methyl t-butyl ether. The equations below show the steps used to make methanol. Determine the oxidation number for each atom in the equation and identify whether the reactions are redox reactions or not. For each redox reaction, identify what is oxidized and what is reduced.

$$
\begin{aligned}
& 3 \mathrm{CH}_4+2 \mathrm{H}_2 \mathrm{O}+\mathrm{CO}_2 \rightarrow 4 \mathrm{CO}+8 \mathrm{H}_2 \\
& \mathrm{CO}+2 \mathrm{H}_2 \rightarrow \mathrm{CH}_3 \mathrm{OH}
\end{aligned}
$$

Zubair Abdulla
Zubair Abdulla
Numerade Educator
05:12

Problem 85

When the calcium carbonate, $\mathrm{CaCO}_3$, in limestone is heated to a high temperature, it decomposes into calcium oxide (called lime or quick lime) and carbon dioxide. Lime was used by the early Romans, Greeks, and Egyptians to make cement and is used today to make over 150 different chemicals. In another reaction, calcium oxide and water form calcium hydroxide, $\mathrm{Ca}(\mathrm{OH})_2$ (called slaked lime), used to remove the sulfur dioxide from smoke stacks above power plants burning high-sulfur coal. The equations for all these reactions are below. Determine the oxidation number for each atom in the equation and identify whether the reactions are redox reaction or not. For each redox reaction, identify what is oxidized and what is reduced.

$$
\begin{aligned}
& \mathrm{CaCO}_3 \xrightarrow{\Delta} \mathrm{CaO}+\mathrm{CO}_2 \\
& \mathrm{CaO}+\mathrm{H}_2 \mathrm{O} \rightarrow \mathrm{Ca}(\mathrm{OH})_2 \\
& \mathrm{SO}_2+\mathrm{H}_2 \mathrm{O} \rightarrow \mathrm{H}_2 \mathrm{SO}_3 \\
& \mathrm{Ca}(\mathrm{OH})_2+\mathrm{H}_2 \mathrm{SO}_3 \rightarrow \mathrm{CaSO}_3+2 \mathrm{H}_2 \mathrm{O}
\end{aligned}
$$

HD
Heather Doyle
Numerade Educator
05:56

Problem 86

Potassium hydroxide, which is used to make fertilizers and soaps, is produced by running an electric current through a potassium chloride solution. The equation for this reaction is below. Is this a redox reaction? What is oxidized, and what is reduced?

$$
2 \mathrm{KCl}(a q)+2 \mathrm{H}_2 \mathrm{O}(l) \rightarrow 2 \mathrm{KOH}(a q)+\mathrm{H}_2(g)+\mathrm{Cl}_2(g)
$$

David Collins
David Collins
Numerade Educator
00:54

Problem 87

The space shuttle's solid rocket boosters get their thrust from the reaction of aluminum metal with ammonium perchlorate, $\mathrm{NH}_4 \mathrm{ClO}_4$, which generates a lot of gas and heat. The billowy white smoke is due to the formation of very finely divided solid aluminum oxide. One of the reactions that takes place is

$$
10 \mathrm{Al}(\mathrm{~s})+6 \mathrm{NH}_4 \mathrm{ClO}_4(\mathrm{~s}) \quad \rightarrow \quad 5 \mathrm{Al}_2 \mathrm{O}_3(\mathrm{~s})+6 \mathrm{HCl}(\mathrm{~g})+3 \mathrm{~N}_2(\mathrm{~g})+9 \mathrm{H}_2 \mathrm{O}(\mathrm{~g})
$$

Is this a redox reaction? What is oxidized, and what is reduced?

Lizabeth Tumminello
Lizabeth Tumminello
Numerade Educator
10:02

Problem 88

For each of the following equations, determine the oxidation number for each atom in the equation and identify whether the reaction is a redox reaction or not. If the reaction is redox, identify what is oxidized, what is reduced, the oxidizing agent, and the reducing agent.
a. $2 \mathrm{HNO}_3(a q)+3 \mathrm{H}_2 \mathrm{~S}(a q) \rightarrow 2 \mathrm{NO}(g)+3 \mathrm{~S}(s)+4 \mathrm{H}_2 \mathrm{O}(l)$
b. $3 \mathrm{CuSO}_4(a q)+2 \mathrm{Na}_3 \mathrm{PO}_4(a q) \rightarrow \mathrm{Cu}_3\left(\mathrm{PO}_4\right)_2(s)+3 \mathrm{Na}_2 \mathrm{SO}_4(a q)$

Emily Wendel
Emily Wendel
Numerade Educator
05:35

Problem 89

Determine the oxidation number for each atom in the following equations and decide whether each reaction is a redox reaction or not. If a reaction is redox, identify which substance is oxidized, which is reduced, the oxidizing agent, and the reducing agent.
a. $\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7(a q)+14 \mathrm{HCl}(a q) \rightarrow 2 \mathrm{KCl}(a q)+2 \mathrm{CrCl}_3(a q)+7 \mathrm{H}_2 \mathrm{O}(l)+3 \mathrm{Cl}_2(g)$
b. $\mathrm{Ca}(s)+2 \mathrm{H}_2 \mathrm{O}(l) \rightarrow \mathrm{Ca}(\mathrm{OH})_2(s)+\mathrm{H}_2(g)$

David Collins
David Collins
Numerade Educator
01:58

Problem 90

Determine the oxidation number for each atom in the following equations and decide whether each reaction is a redox reaction or not. If the reaction is redox, identify which substance is oxidized, which is reduced, the oxidizing agent, and the reducing agent.
a. $2 \mathrm{Ag}_2 \mathrm{CrO}_4(s)+4 \mathrm{HNO}_3(\mathrm{aq}) \rightarrow 4 \mathrm{AgNO}_3(a q)+\mathrm{H}_2 \mathrm{Cr}_2 \mathrm{O}_7(a q)+\mathrm{H}_2 \mathrm{O}(l)$
b. $2 \mathrm{MnO}_4^{-}(\mathrm{aq})+3 \mathrm{IO}_3^{-}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(l) \rightarrow 2 \mathrm{MnO}_2(s)+3 \mathrm{IO}_4^{-}(a q)+2 \mathrm{OH}^{-}(a q)$

David Collins
David Collins
Numerade Educator
01:36

Problem 91

For each of the following equations, determine the oxidation number for each atom in the equation and identify whether the reaction is a redox reaction or not. If the reaction is redox, identify what is oxidized, what is reduced, the oxidizing agent, and the reducing agent.
a. $\mathrm{Ca}(\mathrm{s})+\mathrm{F}_2(\mathrm{~g}) \rightarrow \mathrm{CaF}_2(\mathrm{~s})$
b. $2 \mathrm{Al}(\mathrm{s})+3 \mathrm{H}_2 \mathrm{O}(\mathrm{g}) \rightarrow \mathrm{Al}_2 \mathrm{O}_3(\mathrm{~s})+3 \mathrm{H}_2(\mathrm{~g})$

Lottie Adams
Lottie Adams
Numerade Educator
08:02

Problem 92

Determine the oxidation number for each atom in the following equations and decide whether each reaction is a redox reaction or not. If a reaction is redox, identify which substance is oxidized, which is reduced, the oxidizing agent, and the reducing agent.
a. $\mathrm{Cr}_2 \mathrm{O}_7^{2-}(a q)+6 \mathrm{Cl}^{-}(a q)+14 \mathrm{H}^{+}(a q) \rightarrow 2 \mathrm{Cr}^{3+}(a q)+3 \mathrm{Cl}_2(g)+7 \mathrm{H}_2 \mathrm{O}(l)$
b. $5 \mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4(a q)+2 \mathrm{KMnO}_4(a q)+3 \mathrm{H}_2 \mathrm{SO}_4(a q)$

$$
\rightarrow \quad 10 \mathrm{CO}_2(g)+2 \mathrm{MnSO}_4(a q)+8 \mathrm{H}_2 \mathrm{O}(l)+\mathrm{K}_2 \mathrm{SO}_4(a q)
$$

Bhumika Jayee
Bhumika Jayee
Numerade Educator
02:17

Problem 93

The following equations represent reactions used by the U.S. chemical industry. Classify each with respect to the following categories: combination reaction, decomposition reaction, and single-displacement reaction.
a. $\mathrm{P}_4+5 \mathrm{O}_2+6 \mathrm{H}_2 \mathrm{O} \rightarrow 4 \mathrm{H}_3 \mathrm{PO}_4$
b. $\mathrm{TiCl}_4+\mathrm{O}_2 \rightarrow \mathrm{TiO}_2+2 \mathrm{Cl}_2$
c. $\mathrm{CH}_3 \mathrm{CH}_3(\mathrm{~g}) \xrightarrow{\Delta} \mathrm{CH}_2 \mathrm{CH}_2(\mathrm{~g})+\mathrm{H}_2(\mathrm{~g})$

Daniel Kim
Daniel Kim
Numerade Educator
00:36

Problem 94

The following equations represent reactions used by the U.S. chemical industry. Classify each with respect to the following categories: combination reaction, decomposition reaction, combustion reaction, and single-displacement reaction.
a. $2 \mathrm{HF}+\mathrm{SiF}_4 \rightarrow \mathrm{H}_2 \mathrm{SiF}_6$
b. $2 \mathrm{H}_2 \mathrm{~S}+3 \mathrm{O}_2 \rightarrow 2 \mathrm{SO}_2+2 \mathrm{H}_2 \mathrm{O}$
c. $\mathrm{CH}_3 \mathrm{OH} \xrightarrow{\Delta} \mathrm{CH}_2 \mathrm{O}+\mathrm{H}_2$

Sam Limsuwannarot
Sam Limsuwannarot
Numerade Educator
01:37

Problem 95

Write a balanced equation for the redox reaction of carbon dioxide gas and hydrogen gas to form carbon solid and water vapor.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
02:10

Problem 96

Phosphorus pentachloride, which is used to add chlorine atoms to other substances, can be made from the reaction of phosphorus trichloride and chlorine. The phosphorus pentachloride is the only product. Write a balance equation, without including states, for this redox reaction.

Vishal Sharma
Vishal Sharma
Numerade Educator
03:11

Problem 97

Titanium metal is used to make metal alloys for aircraft, missiles, and artificial hip joints. It is formed in the reaction of titanium(IV) chloride with magnesium metal. The other product is magnesium chloride. Write a balanced equation, without including states, for this redox reaction.

Jennifer Landry
Jennifer Landry
Numerade Educator
02:28

Problem 98

Dichlorine monoxide, which is used to add chlorine atoms to other substances, is made from mercury(II) oxide and chlorine. The products are dichlorine monoxide and mercury. Write a balanced equation, without including states, for this redox reaction.

Crystal Wang
Crystal Wang
Numerade Educator
00:56

Problem 99

Write a balanced equation for the redox reaction of solid potassium with liquid water to form aqueous potassium hydroxide and hydrogen gas.

Keenan Mintz
Keenan Mintz
University of Miami
02:21

Problem 100

Write a balanced equation for the redox reaction of aqueous chlorine with aqueous potassium iodide to form aqueous potassium chloride and solid iodine.

Vishal Sharma
Vishal Sharma
Numerade Educator
02:11

Problem 101

Write a balanced equation for the redox reaction of calcium metal and bromine liquid to form solid calcium bromide.

Vishal Sharma
Vishal Sharma
Numerade Educator
01:52

Problem 102

Write a balanced equation for the redox reaction of solid copper(II) sulfide with oxygen gas to form solid copper(II) oxide and sulfur dioxide gas.

David Collins
David Collins
Numerade Educator
03:21

Problem 103

Magnesium chloride is used to make disinfectants, fire extinguishers, paper, and floor sweeping compounds. It is made from the redox reaction of hydrochloric acid with solid magnesium hydroxide. Write a balanced equation for this reaction, which yields aqueous magnesium chloride and liquid water.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
00:55

Problem 104

Write a balanced equation for the redox reaction at room temperature of chromium metal with hydrochloric acid to form aqueous chromium(III) chloride and hydrogen gas.

Aadit Sharma
Aadit Sharma
Numerade Educator
00:31

Problem 105

What makes one battery better than another? Find a reference book that tells you about the properties of the elements. Why do you think lithium batteries are superior to batteries that use lead? What other elements might be considered for new batteries?

Aadit Sharma
Aadit Sharma
Numerade Educator