Chemistry: An Introduction to General, Organic, and Biological Chemistry

Problem 7

Oxepine $\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}\right)$ is a seven-membered ring oxacycle.
a. How many moles of carbon are present in 1.0 millimole of oxepine?
b. How many moles of $\mathrm{H}$ are present in 1 mole of oxepine?
c. How many moles of $\mathrm{O}$ are present in 5 moles of oxepine?

David Collins

Numerade Educator

02:41

Problem 8

Aluminum sulfate, $\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3},$ is used in some antiperspirants.
a. How many moles of $\mathrm{O}$ are present in $3.0 \mathrm{moles}$ of $\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3} ?$
b. How many moles of aluminum ions $\left(\mathrm{Al}^{3+}\right)$ are present in 0.40 mole of $\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3} ?$
c. How many moles of sulfate ions $\left(\mathrm{SO}_{4}^{2-}\right)$ are present in 1.5 moles of $\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3} ?$

Chareen Guzman

Numerade Educator

05:30

Problem 9

Naproxen, found in Aleve, is used to treat the pain and inflammation caused by arthritis. Naproxen has a formula of $\mathrm{C}_{14} \mathrm{H}_{14} \mathrm{O}_{3}$.
a. How many moles of $\mathrm{C}$ are present in 2.30 moles of naproxen?
b. How many moles of $\mathrm{H}$ are present in 0.444 mole of naproxen?
c. How many moles of $\mathrm{O}$ are present in $0.0765 \mathrm{~mole}$ of naproxen?

Vishal Sharma

Numerade Educator

04:38

Problem 10

Benadryl is an over-the-counter drug used to treat allergy symptoms. The formula of Benadryl is $\mathrm{C}_{17} \mathrm{H}_{21} \mathrm{NO}$.
a. How many moles of $\mathrm{C}$ are present in $0.733 \mathrm{~mole}$ of Benadryl?
b. How many moles of $\mathrm{H}$ are present in 2.20 moles of Benadryl?
c. How many moles of $\mathrm{N}$ are present in 1.54 moles of Benadryl?

Vishal Sharma

Numerade Educator

08:41

Problem 11

Calculate the molar mass for each of the following:
a. $\mathrm{Cl}_{2}$
b. $\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}_{3}$
c. $\mathrm{Mg}_{3}\left(\mathrm{PO}_{4}\right)_{2}$

Madeleine Sarner

Numerade Educator

07:02

Problem 12

Calculate the molar mass for each of the following:
a. $\mathrm{O}_{2}$
b. $\mathrm{KH}_{2} \mathrm{PO}_{4}$
c. $\mathrm{Fe}\left(\mathrm{ClO}_{4}\right)_{3}$

Madeleine Sarner

Numerade Educator

05:47

Problem 13

Calculate the molar mass for each of the following:
a. $\mathrm{Br}_{2}$
b. $\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O}$
c. $\mathrm{CuSO}_{4}$
d. $B F_{3}$
e. $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{Cl}$

Madeleine Sarner

Numerade Educator

04:47

Problem 14

Calculate the molar mass for each of the following:
a. $\mathrm{C}_{4} \mathrm{H}_{8} \mathrm{O}_{4}$
b. $\mathrm{Ga}_{2}\left(\mathrm{CO}_{3}\right)_{3}$
c. $\mathrm{KBrO}_{4}$

Madeleine Sarner

Numerade Educator

01:28

Problem 15

Calculate the number of grams in each of the following:
a. 2.0 moles of $\mathrm{MgCl}_{2}$
b. 3.5 moles of benzene $\mathrm{C}_{6} \mathrm{H}_{6}$
c. 5.00 moles of $\mathrm{NaOMe}$
d. 0.5 mole of $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$

David Collins

Numerade Educator

06:01

Problem 16

Calculate the molar mass for each of the following:
a. $\mathrm{FeSO}_{4}$, iron supplement
b. $\mathrm{Al}_{2} \mathrm{O}_{3},$ absorbent and abrasive
c. $\mathrm{C}_{7} \mathrm{H}_{5} \mathrm{NO}_{3} \mathrm{~S},$ saccharin, artificial sweetener

Madeleine Sarner

Numerade Educator

07:11

Problem 17

Calculate the molar mass for each of the following:
a. $\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3},$ antiperspirant
b. $\mathrm{KC}_{4} \mathrm{H}_{5} \mathrm{O}_{6},$ cream of tartar
c. $\mathrm{C}_{16} \mathrm{H}_{19} \mathrm{~N}_{3} \mathrm{O}_{5} \mathrm{~S},$ amoxicillin, antibiotic

Madeleine Sarner

Numerade Educator

05:58

Problem 18

Calculate the molar mass for each of the following:
a. $\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O},$ rubbing alcohol
b. $\left(\mathrm{NH}_{4}\right)_{2} \mathrm{CO}_{3},$ baking powder
c. $\mathrm{Zn}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2},$ zinc supplement

Madeleine Sarner

Numerade Educator

07:06

Problem 19

Calculate the molar mass for each of the following:
a. $\mathrm{C}_{8} \mathrm{H}_{9} \mathrm{NO}_{2},$ acetaminophen used in Tylenol
b. $\mathrm{Ca}_{3}\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}\right)_{2},$ calcium supplement
c. $\mathrm{C}_{17} \mathrm{H}_{18} \mathrm{FN}_{3} \mathrm{O}_{3},$ Cipro, used to treat a range of bacterial infections

Madeleine Sarner

Numerade Educator

07:12

Problem 20

Calculate the molar mass for each of the following:
a. $\mathrm{CaSO}_{4},$ calcium sulfate, used to make casts to protect broken bones
b. $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{~N}_{2} \mathrm{O}_{4} \mathrm{Pt},$ Carboplatin, used in chemotherapy
c. $\mathrm{C}_{12} \mathrm{H}_{18} \mathrm{O},$ Propofol, used to induce anesthesia during surgery

Madeleine Sarner

Numerade Educator

01:41

Problem 21

Calculate the mass, in grams, for each of the following:
a. 1.50 moles of Na
b. 2.80 moles of Ca
c. 0.125 mole of $\mathrm{CO}_{2}$
d. 0.0485 mole of $\mathrm{Na}_{2} \mathrm{CO}_{3}$
e. $7.14 \times 10^{2}$ moles of $\mathrm{PCl}_{3}$

David Collins

Numerade Educator

01:40

Problem 22

Calculate the mass, in grams, for each of the following:
a. 5.12 moles of $\mathrm{Al}$
b. 0.75 mole of Cu
c. 3.52 moles of $\mathrm{MgBr}_{2}$
d. 0.145 mole of $\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}$
e. 2.08 moles of $\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}$

David Collins

Numerade Educator

01:13

Problem 23

How many moles of $\mathrm{O}$ are present in each of the following quantities?
a. $23 \mathrm{~g}$ of $\mathrm{O}$
b. $110 \mathrm{~g}$ of $\mathrm{CO}_{2}$
c. 4.0 moles of $\mathrm{Al}_{2} \mathrm{O}_{3}$

David Collins

Numerade Educator

01:48

Problem 24

How many moles of $\mathrm{O}$ are present in each of the following quantities?
a. $88 \mathrm{~g}$ of $\mathrm{CO}_{2}$
$\begin{array}{ll}\text { b. } 0.25 \mathrm{~kg} \text { of } \mathrm{NO}_{2} & \text { c. } 100 \mathrm{~g} \text { ice }\end{array}$

David Collins

Numerade Educator

08:24

Problem 25

How many moles are contained in each of the following?
a. $25.0 \mathrm{~g}$ of $\mathrm{Cu}$
b. $0.600 \mathrm{~g}$ of $\mathrm{P}$
c. $12.0 \mathrm{~g}$ of $\mathrm{CO}$
d. $60.5 \mathrm{~g}$ of $\mathrm{CH}_{4}$

Madeleine Sarner

Numerade Educator

View

Problem 26

Calculate the number of moles in each of the following:
a. $85.2 \mathrm{~g}$ of $\mathrm{Ni}$
b. $144 \mathrm{~g}$ of $\mathrm{K}$
c. $6.4 \mathrm{~g}$ of $\mathrm{H}_{2} \mathrm{O}$
d. $308 \mathrm{~g}$ of $\mathrm{BaSO}_{4}$
e. $252.8 \mathrm{~g}$ of fructose, $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$

Ronald Prasad

Numerade Educator

01:25

Problem 27

Calculate the number of moles in $15.0 \mathrm{~g}$ of each of the following:
a. $\mathrm{Ar}$
b. $\mathrm{N}_{2}$
c. $\mathrm{Fe}_{2} \mathrm{O}_{3}$
d. $\mathrm{CaCl}_{2}$

David Collins

Numerade Educator

01:38

Problem 28

Calculate the number of moles in $4.00 \mathrm{~g}$ of each of the following:
a. Au
b. $\mathrm{SnO}_{2}$
c. $\mathrm{CS}_{2}$
d. $\mathrm{Ca}_{3} \mathrm{~N}_{2}$
e. $\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{6},$ vitamin $\mathrm{C}$

David Collins

Numerade Educator

01:09

Problem 29

Chloroethane, $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{Cl}$, is used to diagnose dead tooth nerves.
a. How many moles are in $34.0 \mathrm{~g}$ of chloroethane?
b. How many grams are in 1.50 moles of chloroethane?

David Collins

Numerade Educator

Problem 30

Allyl sulfide, $\left(\mathrm{C}_{3} \mathrm{H}_{5}\right)_{2} \mathrm{~S},$ gives garlic, onions, and leeks their characteristic odor.
a. How many moles are in $23.2 \mathrm{~g}$ of allyl sulfide?
b. How many grams are in 0.75 mole of allyl sulfide?

David Collins

Numerade Educator

Problem 31

a. The compound $\mathrm{MgSO}_{4}$, Epsom salts, is used to soothe sore feet and muscles. How many grams will you need to prepare a bath containing 5.00 moles of Epsom salts?
b. Potassium iodide, KI, is used as an expectorant. How many grams are in 0.450 mole of potassium iodide?

David Collins

Numerade Educator

01:40

Problem 32

a. Cyclopropane, $\mathrm{C}_{3} \mathrm{H}_{6}$, is an anesthetic given by inhalation. How many grams are in 0.25 mole of cyclopropane?
b. The sedative Demerol hydrochloride has the formula $\mathrm{C}_{15} \mathrm{H}_{22} \mathrm{ClNO}_{2}$. How many grams are in $0.025 \mathrm{~mole}$ of
Demerol hydrochloride?

Rithvik Manne

Numerade Educator

01:53

Problem 33

Methyl salicylate or oil of wintergreen $\left(\mathrm{C}_{8} \mathrm{H}_{8} \mathrm{O}_{3}\right)$ is an organic ester widely used as a fragrance in foods $\&$ beverages and in liniments.
a. How many grams of the compound are there in 1.75 moles of methyl salicylate?
b. How many moles of the compound are there in $42.0 \mathrm{~g}$ of methyl salicylate?
c. How many grams of $\mathrm{O}$ are present in $42.0 \mathrm{~g}$ of methyl salicylate?

David Collins

Numerade Educator

Problem 34

Chloroform, CHCl $_{3}$, was formerly used as an anesthetic but its use was discontinued due to respiratory and cardiac failure.
a. How many grams are in 0.122 mole of chloroform?
b. How many moles are in $26.7 \mathrm{~g}$ of chloroform?

David Collins

Numerade Educator

01:43

Problem 35

Determine whether each of the following chemical equations is balanced or not balanced:
a. $\mathrm{S}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{SO}_{3}(g)$
b. $2 \mathrm{Ga}(s)+3 \mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{GaCl}_{3}(s)$
c. $\mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{H}_{2} \mathrm{O}(g)$
d. $\mathrm{C}_{3} \mathrm{H}_{8}(g)+5 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 3 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)$

David Collins

Numerade Educator

01:19

Problem 36

Determine whether each of the following chemical equations is balanced or not balanced:
a. $\mathrm{PCl}_{3}(s)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{PCl}_{5}(s)$
b. $\mathrm{CO}(g)+2 \mathrm{H}_{2}(g) \longrightarrow \mathrm{CH}_{4} \mathrm{O}(g)$
c. $2 \mathrm{KClO}_{3}(s) \longrightarrow 2 \mathrm{KCl}(s)+\mathrm{O}_{2}(g)$
d. $\mathrm{Mg}(s)+\mathrm{N}_{2}(g) \longrightarrow \mathrm{Mg}_{3} \mathrm{~N}_{2}(s)$

David Collins

Numerade Educator

01:35

Problem 37

Balance each of the following chemical equations:
a. $\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{NO}(g)$
b. $\mathrm{HgO}(s) \stackrel{\Delta}{\longrightarrow} \mathrm{Hg}(l)+\mathrm{O}_{2}(g)$
c. $\mathrm{Fe}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{Fe}_{2} \mathrm{O}_{3}(s)$
d. $\mathrm{Na}(s)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{NaCl}(s)$

Narayan Hari

Numerade Educator

01:50

Problem 38

Balance each of the following chemical equations:
a. $\mathrm{Mg}(s)+\mathrm{Br}_{2}(l) \longrightarrow \mathrm{MgBr}_{2}(s)$
b. $\mathrm{O}_{2}(g)+\mathrm{P}_{4}(s) \longrightarrow \mathrm{P}_{4} \mathrm{O}_{10}(s)$
c. $\mathrm{K}_{2} \mathrm{CO}_{3}(s)+\mathrm{HCl}(a q) \longrightarrow \mathrm{KCl}(a q)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CO}_{2}(s)$
d. $\mathrm{Zn}(s)+\mathrm{HCl}(a q) \longrightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{H}_{2}(g)$

David Collins

Numerade Educator

02:29

Problem 39

Balance each of the following chemical equations:
a. $\mathrm{Mg}(s)+\mathrm{AgNO}_{3}(a q) \longrightarrow \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{Ag}(s)$
b. $\mathrm{Al}(s)+\mathrm{CuSO}_{4}(a q) \longrightarrow \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)+\mathrm{Cu}(s)$
c. $\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{NaCl}(a q) \longrightarrow \mathrm{PbCl}_{2}(s)+\mathrm{NaNO}_{3}(a q)$
d. $\mathrm{Al}(s)+\mathrm{HCl}(a q) \longrightarrow \mathrm{H}_{2}(g)+\mathrm{AlCl}_{3}(a q)$

David Collins

Numerade Educator

01:58

Problem 40

Balance each of the following chemical equations:
a. $\mathrm{Zn}(s)+\mathrm{HNO}_{3}(a q) \longrightarrow \mathrm{H}_{2}(g)+\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}(a q)$
b. $\mathrm{Al}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{H}_{2}(g)+\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)$
c. $\mathrm{K}_{2} \mathrm{SO}_{4}(a q)+\mathrm{BaCl}_{2}(a q) \longrightarrow \mathrm{BaSO}_{4}(s)+\mathrm{KCl}(a q)$
d. $\mathrm{CaCO}_{3}(s) \longrightarrow \mathrm{CaO}(s)+\mathrm{CO}_{2}(g)$

David Collins

Numerade Educator

01:36

Problem 41

Classify each of the following as a combination, decomposition, single replacement, double replacement, or combustion reaction:
a. $2 \mathrm{Al}_{2} \mathrm{O}_{3}(s) \stackrel{\Delta}{\longrightarrow} 4 \mathrm{Al}(s)+3 \mathrm{O}_{2}(g)$
b. $\mathrm{Br}_{2}(l)+\mathrm{BaI}_{2}(s) \longrightarrow \mathrm{BaBr}_{2}(s)+\mathrm{I}_{2}(s)$
c. $2 \mathrm{C}_{2} \mathrm{H}_{2}(g)+5 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 4 \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)$
d. $\mathrm{BaCl}_{2}(a q)+\mathrm{K}_{2} \mathrm{CO}_{3}(a q) \longrightarrow \mathrm{BaCO}_{3}(s)+2 \mathrm{KCl}(a q)$
e. $\mathrm{Pb}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{PbO}_{2}(s)$

David Collins

Numerade Educator

01:23

Problem 42

Classify each of the following as a combination, decomposition, single replacement, double replacement, or combustion reaction:
a. $\mathrm{H}_{2}(g)+\mathrm{Br}_{2}(l) \longrightarrow 2 \mathrm{HBr}(g)$
b. $\mathrm{AgNO}_{3}(a q)+\mathrm{NaCl}(a q) \longrightarrow \mathrm{AgCl}(s)+\mathrm{NaNO}_{3}(a q)$
c. $2 \mathrm{H}_{2} \mathrm{O}_{2}(a q) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{O}_{2}(g)$
d. $\mathrm{Zn}(s)+\mathrm{CuCl}_{2}(a q) \longrightarrow \mathrm{Cu}(s)+\mathrm{ZnCl}_{2}(a q)$
e. $\mathrm{C}_{5} \mathrm{H}_{8}(g)+7 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 5 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)$

David Collins

Numerade Educator

01:24

Problem 43

Classify each of the following as a combination, decomposition, single replacement, double replacement, or combustion reaction:
a. $4 \mathrm{Fe}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Fe}_{2} \mathrm{O}_{3}(s)$
b. $\mathrm{Mg}(s)+2 \mathrm{AgNO}_{3}(a q) \longrightarrow 2 \mathrm{Ag}(s)+\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}(a q)$
c. $\mathrm{CuCO}_{3}(s) \stackrel{\Delta}{\longrightarrow} \mathrm{CuO}(s)+\mathrm{CO}_{2}(g)$
d. $\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)+6 \mathrm{KOH}(a q) \longrightarrow$
$$
2 \mathrm{Al}(\mathrm{OH})_{3}(s)+3 \mathrm{~K}_{2} \mathrm{SO}_{4}(a q)
$$
e. $\mathrm{C}_{4} \mathrm{H}_{8}(g)+6 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 4 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)$

David Collins

Numerade Educator

01:16

Problem 44

Classify each of the following as a combination, decomposition, single replacement, double replacement, or combustion reaction:
$$
\begin{array}{l}
\text { a. } \mathrm{HCl}(a q)+\mathrm{NaOH}(a q) \longrightarrow \mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \\
\text { b. } 2 \mathrm{Na}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{H}_{2}(g)+2 \mathrm{NaOH}(a q) \\
\text { c. } \mathrm{Ca}(s)+2 \mathrm{AuNO}_{3}(a q) \longrightarrow \mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}(a q)+2 \mathrm{Au}(s) \\
\text { d. } 4 \mathrm{Al}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Al}_{2} \mathrm{O}_{3}(s) \\
\text { e. } \mathrm{C}_{2} \mathrm{H}_{6}(g)+3 \mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{CO}(g) \\
\quad+3 \mathrm{H}_{2} \mathrm{O}+\text { energy }
\end{array}
$$

David Collins

Numerade Educator

01:06

Problem 45

Identify each of the following as an oxidation or a reduction:
a. $\mathrm{Na}^{+}(a q)+e^{-} \longrightarrow \mathrm{Na}(s)$
b. $\mathrm{Ni}(s) \longrightarrow \mathrm{Ni}^{2+}(a q)+2 e^{-}$
c. $\mathrm{Cr}^{3+}(a q)+3 e^{-} \longrightarrow \mathrm{Cr}(s)$
d. $2 \mathrm{H}^{+}(a q)+2 e^{-} \longrightarrow \mathrm{H}_{2}(g)$

David Collins

Numerade Educator

01:17

Problem 46

Identify each of the following as an oxidation or a reduction:
a. $\mathrm{O}_{2}(g)+4 e^{-} \longrightarrow 2 \mathrm{O}^{2-}(a q)$
b. $\operatorname{Ag}(s) \longrightarrow \operatorname{Ag}^{+}(a q)+e^{-}$
c. $\mathrm{Fe}^{3+}(a q)+e^{-} \longrightarrow \mathrm{Fe}^{2+}(a q)$
d. $2 \mathrm{Br}^{-}(a q) \longrightarrow \mathrm{Br}_{2}(l)+2 e^{-}$

David Collins

Numerade Educator

02:06

Problem 47

In each of the following, identify the reactant that is oxidized and the reactant that is reduced:
a. $\mathrm{Zn}(s)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{ZnCl}_{2}(s)$
b. $\mathrm{Cl}_{2}(g)+2 \mathrm{NaBr}(a q) \longrightarrow 2 \mathrm{NaCl}(a q)+\mathrm{Br}_{2}(l)$
c. $2 \mathrm{PbO}(s) \longrightarrow 2 \mathrm{~Pb}(s)+\mathrm{O}_{2}(g)$
d. $2 \mathrm{Fe}^{3+}(a q)+\mathrm{Sn}^{2+}(a q) \longrightarrow 2 \mathrm{Fe}^{2+}(a q)+\mathrm{Sn}^{4+}(a q)$

David Collins

Numerade Educator

01:51

Problem 48

In each of the following, identify the reactant that is oxidized and the reactant that is reduced:
a. $2 \mathrm{Li}(s)+\mathrm{F}_{2}(g) \longrightarrow 2 \mathrm{LiF}(s)$
b. $\mathrm{Cl}_{2}(g)+2 \mathrm{KI}(a q) \longrightarrow \mathrm{I}_{2}(s)+2 \mathrm{KCl}(a q)$
c. $2 \mathrm{Al}(s)+3 \mathrm{Sn}^{2+}(a q) \longrightarrow 3 \mathrm{Sn}(s)+2 \mathrm{Al}^{3+}(a q)$
d. $\mathrm{Fe}(s)+\mathrm{CuSO}_{4}(a q) \longrightarrow \mathrm{Cu}(s)+\mathrm{FeSO}_{4}(a q)$

David Collins

Numerade Educator

Problem 49

In the mitochondria of human cells, energy is provided by the oxidation and reduction reactions of the iron ions in the cytochromes in electron transport. Identify each of the following as an oxidation or a reduction:
a. $\mathrm{Fe}^{3+}+e^{-} \longrightarrow \mathrm{Fe}^{2+}$
b. $\mathrm{Fe}^{2+} \longrightarrow \mathrm{Fe}^{3+}+e^{-}$

David Collins

Numerade Educator

01:12

Problem 50

Chlorine $\left(\mathrm{Cl}_{2}\right)$ is a strong germicide used to disinfect drinking water and to kill microbes in swimming pools. If the product is $\mathrm{Cl}^{-}$, was the elemental chlorine oxidized or reduced?

David Collins

Numerade Educator

Problem 51

When olefin, an unsaturated hydrocarbon, reacts with hydrogen, it forms a saturated hydrocarbon. Is olefin oxidized or reduced in the hydrogenation reaction?
$$
\mathrm{C}_{8} \mathrm{H}_{16}+\mathrm{H}_{2} \longrightarrow \mathrm{C}_{8} \mathrm{H}_{18}
$$

David Collins

Numerade Educator

01:22

Problem 52

In one of the reactions in the citric acid cycle, which provides energy, succinic acid is converted to fumaric acid.
$$
\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{4} \longrightarrow \mathrm{C}_{4} \mathrm{H}_{4} \mathrm{O}_{4}+2 \mathrm{H}
$$
Succinic acid Fumaric acid
The reaction is accompanied by a coenzyme, flavin adenine dinucleotide (FAD).
$$
\mathrm{FAD}+2 \mathrm{H} \longrightarrow \mathrm{FADH}_{2}
$$
a. Is succinic acid oxidized or reduced?
b. Is FAD oxidized or reduced?
c. Why would the two reactions occur together?

David Collins

Numerade Educator

Problem 53

Write all of the mole-mole factors for each of the following chemical equations:
a. $2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{SO}_{3}(g)$
b. $4 \mathrm{P}(s)+5 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{P}_{2} \mathrm{O}_{5}(s)$

David Collins

Numerade Educator

Problem 54

Write all of the mole-mole factors for each of the following chemical equations:
a. $2 \mathrm{Al}(s)+3 \mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{AlCl}_{3}(s)$
b. $4 \mathrm{HCl}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Cl}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)$

David Collins

Numerade Educator

02:48

Problem 55

The chemical reaction of hydrogen with oxygen produces water.
$$
2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(g)
$$
a. How many moles of $\mathrm{O}_{2}$ are required to react with 2.6 moles of $\mathrm{H}_{2} ?$
b. How many moles of $\mathrm{H}_{2}$ are needed to react with $5.0 \mathrm{moles}$ of $\mathrm{O}_{2} ?$
c. How many moles of $\mathrm{H}_{2} \mathrm{O}$ form when 2.5 moles of $\mathrm{O}_{2}$ reacts?

Vishal Sharma

Numerade Educator

03:20

Problem 56

Ammonia is produced by the chemical reaction of hydrogen and nitrogen.
$$
\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow \begin{array}{l}
2 \mathrm{NH}_{3}(g) \\
\text { Ammonia }
\end{array}
$$
a. How many moles of $\mathrm{H}_{2}$ are needed to react with 1.8 moles of $\mathrm{N}_{2} ?$
b. How many moles of $\mathrm{N}_{2}$ reacted if $0.60 \mathrm{~mole}$ of $\mathrm{NH}_{3}$ is produced?
c. How many moles of $\mathrm{NH}_{3}$ are produced when 1.4 moles of $\mathrm{H}_{2}$ reacts?

Anna D.

Numerade Educator

01:41

Problem 57

Carbon disulfide and carbon monoxide are produced when carbon is heated with sulfur dioxide.
$$
5 \mathrm{C}(s)+2 \mathrm{SO}_{2}(g) \stackrel{\Delta}{\longrightarrow} \mathrm{CS}_{2}(l)+4 \mathrm{CO}(g)
$$
a. How many moles of $\mathrm{C}$ are needed to react with $0.500 \mathrm{~mole}$ of $\mathrm{SO}_{2} ?$
b. How many moles of CO are produced when 1.2 moles of $\mathrm{C}$ reacts?
c. How many moles of $\mathrm{SO}_{2}$ are needed to produce $0.50 \mathrm{~mole}$ of $\mathrm{CS}_{2} ?$
d. How many moles of $\mathrm{CS}_{2}$ are produced when $2.5 \mathrm{moles}$ of C reacts?

David Collins

Numerade Educator

02:38

Problem 58

Write a balanced equation for the complete combustion of ethane $\left(\mathrm{C}_{2} \mathrm{H}_{6}\right)$
a. How many moles of water are produced when $10 \mathrm{mmol}$ of ethane reacts in the above combustion?
b. What if the amount of oxygen is not enough for the ethane to combust?
c. Give a balanced equation if there are only two equivalents of oxygen available for the combustion.

David Collins

Numerade Educator

01:30

Problem 59

Sodium reacts with oxygen to produce sodium oxide.
$$
4 \mathrm{Na}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Na}_{2} \mathrm{O}(s)
$$
a. How many grams of $\mathrm{Na}_{2} \mathrm{O}$ are produced when $57.5 \mathrm{~g}$ of Na reacts?
b. If you have $18.0 \mathrm{~g}$ of $\mathrm{Na}$, how many grams of $\mathrm{O}_{2}$ are needed for the reaction?
c. How many grams of $\mathrm{O}_{2}$ are needed in a reaction that produces $75.0 \mathrm{~g}$ of $\mathrm{Na}_{2} \mathrm{O} ?$

Ma Ednelyn Lim

Numerade Educator

01:52

Problem 60

Nitrogen gas reacts with hydrogen gas to produce ammonia.
$$
\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)
$$
a. If you have $3.64 \mathrm{~g}$ of $\mathrm{H}_{2}$, how many grams of $\mathrm{NH}_{3}$ can be produced?
b. How many grams of $\mathrm{H}_{2}$ are needed to react with $2.80 \mathrm{~g}$ of $\mathrm{N}_{2} ?$
c. How many grams of $\mathrm{NH}_{3}$ can be produced from $12.0 \mathrm{~g}$ of $\mathrm{H}_{2} ?$

David Collins

Numerade Educator

01:49

Problem 62

Iron(III) oxide reacts with carbon to give iron and carbon monoxide.
$$
\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{C}(s) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{CO}(g)
$$
a. How many grams of $\mathrm{C}$ are required to react with $16.5 \mathrm{~g}$ of $\mathrm{Fe}_{2} \mathrm{O}_{3} ?$
b. How many grams of $\mathrm{CO}$ are produced when $36.0 \mathrm{~g}$ of $\mathrm{C}$ reacts?
c. How many grams of Fe can be produced when $6.00 \mathrm{~g}$ of $\mathrm{Fe}_{2} \mathrm{O}_{3}$ reacts?

David Collins

Numerade Educator

02:11

Problem 63

Nitrogen dioxide and water react to produce nitric acid, $\mathrm{HNO}_{3}$, and nitrogen oxide.
$$
3 \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{HNO}_{3}(a q)+\mathrm{NO}(g)
$$
a. How many grams of $\mathrm{H}_{2} \mathrm{O}$ are needed to react with $28.0 \mathrm{~g}$ of $\mathrm{NO}_{2} ?$
b. How many grams of NO are produced from $15.8 \mathrm{~g}$ of $\mathrm{H}_{2} \mathrm{O} ?$
c. How many grams of $\mathrm{HNO}_{3}$ are produced from $8.25 \mathrm{~g}$ of $\mathrm{NO}_{2} ?$

David Collins

Numerade Educator

13:37

Problem 64

Calcium cyanamide, $\mathrm{CaCN}_{2}$, reacts with water to form calcium carbonate and ammonia.
$$
\mathrm{CaCN}_{2}(s)+3 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{CaCO}_{3}(s)+2 \mathrm{NH}_{3}(g)
$$
a. How many grams of $\mathrm{H}_{2} \mathrm{O}$ are needed to react with $75.0 \mathrm{~g}$ of $\mathrm{CaCN}_{2} ?$
b. How many grams of $\mathrm{NH}_{3}$ are produced from $5.24 \mathrm{~g}$ of $\mathrm{CaCN}_{2} ?$
c. How many grams of $\mathrm{CaCO}_{3}$ form if $155 \mathrm{~g}$ of $\mathrm{H}_{2} \mathrm{O}$ reacts?

Noah Boudrie

Numerade Educator

04:32

Problem 65

When solid lead(II) sulfide reacts with oxygen gas, the products are solid lead(II) oxide and sulfur dioxide gas.
a. Write the balanced chemical equation for the reaction.
b. How many grams of oxygen are required to react with $29.9 \mathrm{~g}$ of lead(II) sulfide?
c. How many grams of sulfur dioxide can be produced when $65.0 \mathrm{~g}$ of lead(II) sulfide reacts?
d. How many grams of lead(II) sulfide are used to produce $128 \mathrm{~g}$ of lead(II) oxide?

David Collins

Numerade Educator

01:58

Problem 66

Aluminum oxidizes to form aluminum oxide.
a. Write the balanced chemical equation for the reaction.
b. How many mmol and grams of aluminum are needed to react with 6 mmol of oxygen?
c. How many moles and grams of aluminum oxide are produced with 4 mole of aluminum?

David Collins

Numerade Educator

01:05

Problem 67

a. Why do chemical reactions require energy of activation?
b. In an exothermic reaction, is the energy of the products higher or lower than that of the reactants?
c. Draw an energy diagram for an exothermic reaction.

David Collins

Numerade Educator

01:25

Problem 68

a. What is measured by the heat of reaction?
b. In an endothermic reaction, is the energy of the products higher or lower than that of the reactants?
c. Draw an energy diagram for an endothermic reaction.

David Collins

Numerade Educator

Problem 69

Classify each of the following as exothermic or endothermic:
a. A reaction releases $550 \mathrm{~kJ}$.
b. The energy level of the products is higher than that of the reactants.
c. The metabolism of glucose in the body provides energy.

David Collins

Numerade Educator

01:26

Problem 70

Classify each of the following as exothermic or endothermic:
a. The energy level of the products is lower than that of the reactants.
b. In the body, the synthesis of proteins requires energy.
c. A reaction absorbs $125 \mathrm{~kJ}$.

David Collins

Numerade Educator

Problem 71

Classify each of the following as exothermic or endothermic:
a. $\mathrm{CH}_{4}(g)+2 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)+802 \mathrm{~kJ}$
b. $\mathrm{Ca}(\mathrm{OH})_{2}(s)+65.3 \mathrm{~kJ} \longrightarrow \mathrm{CaO}(s)+\mathrm{H}_{2} \mathrm{O}(l)$
c. $2 \mathrm{Al}(s)+\mathrm{Fe}_{2} \mathrm{O}_{3}(s) \longrightarrow \mathrm{Al}_{2} \mathrm{O}_{3}(s)+2 \mathrm{Fe}(s)+850 \mathrm{~kJ}$

David Collins

Numerade Educator

01:09

Problem 72

Classify each of the following as exothermic or endothermic:
a. $\mathrm{C}_{3} \mathrm{H}_{8}(g)+5 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 3 \mathrm{C} \mathrm{O}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)+2220 \mathrm{~kJ}$
b. $2 \mathrm{Na}(s)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{NaCl}(s)+819 \mathrm{~kJ}$
c. $\mathrm{PCl}_{5}(g)+67 \mathrm{~kJ} \longrightarrow \mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g)$

David Collins

Numerade Educator

01:34

Problem 73

a. What is meant by the rate of a reaction?
b. Why does bread grow mold more quickly at room temperature than in the refrigerator?

David Collins

Numerade Educator

01:17

Problem 74

a. How does a catalyst affect the activation energy?
b. Why is pure oxygen used in respiratory distress?

David Collins

Numerade Educator

Problem 75

How would each of the following change the rate of the reaction shown here?
$$
2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{SO}_{3}(g)
$$
a. adding some $\mathrm{SO}_{2}(g)$
b. increasing the temperature
c. adding a catalyst
d. removing some $\mathrm{O}_{2}(g)$

David Collins

Numerade Educator

01:13

Problem 76

How would each of the following change the rate of the reaction shown here?
$$
2 \mathrm{NO}(g)+2 \mathrm{H}_{2}(g) \longrightarrow \mathrm{N}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)
$$
a. adding some $\mathrm{NO}(g)$
b. decreasing the temperature
c. removing some $\mathrm{H}_{2}(g)$
d. adding a catalyst

David Collins

Numerade Educator

Problem 77

a. During cellular respiration, aqueous $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$ (glucose) in the cells undergoes a reaction with oxygen gas to form gaseous carbon dioxide and liquid water. Write and balance the chemical equation for reaction of glucose in the human body.
b. In plants, carbon dioxide gas and liquid water are converted to aqueous glucose $\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)$ and oxygen gas. Write and balance the chemical equation for production of glucose in plants.

David Collins

Numerade Educator

02:00

Problem 78

Fatty acids undergo reaction with oxygen gas and form gaseous carbon dioxide and liquid water when utilized for energy in the body.
a. Write and balance the equation for the combustion of the fatty acid aqueous capric acid, $\mathrm{C}_{10} \mathrm{H}_{20} \mathrm{O}_{2}$.
b. Write and balance the equation for the combustion of the fatty acid aqueous myristic acid, $\mathrm{C}_{14} \mathrm{H}_{28} \mathrm{O}_{2}$.

David Collins

Numerade Educator

01:17

Problem 79

Using the models of the molecules (black $=\mathrm{C},$ white $=\mathrm{H}$, yellow $=\mathrm{S},$ green $=\mathrm{Cl}$ ), determine each of the following for models of compounds 1 and 2:(7.1,7.2,7.3)
a. molecular formula
b. molar mass
c. number of moles in $10.0 \mathrm{~g}$

David Collins

Numerade Educator

01:49

Problem 80

Using the models of the molecules (black $=\mathrm{C},$ white $=\mathrm{H},$ yellow $=\mathrm{S},$ red $=\mathrm{O}$ ), determine each of the following for models of compounds 1 and 2:(7.1,7.2,7.3)
a. molecular formula
b. molar mass
c. number of moles in $10.0 \mathrm{~g}$

David Collins

Numerade Educator

04:52

Problem 81

A dandruff shampoo contains dipyrithione, an antibacterial and antifungal agent, which has the empirical formula $\mathrm{C}_{5} \mathrm{H}_{4} \mathrm{NOS}$. (7.1,7.2,7.3,7.4,7.5)
a. What is the mass of the empirical formula of dipyrithione?
b. If the molar mass of dipyrithione is $252.31 \mathrm{~g},$ what is its molecular formula?
c. What is the mass percent of S in dipyrithione?
d. How many grams of $\mathrm{H}$ are there in $10.0 \mathrm{~g}$ of dipyrithione?
e. What is the weight of $1.5 \times 10^{-3} \mathrm{~mol}$ of dipyrithione?

David Collins

Numerade Educator

05:17

Problem 82

Ibuprofen, an anti-inflammatory drug in Advil, has the formula $\mathrm{C}_{13} \mathrm{H}_{18} \mathrm{O}_{2} .(7.1,7.2,7.3)$
a. What is the molar mass of ibuprofen?
b. How many grams of ibuprofen are in 0.525 mole?
c. How many moles of $\mathrm{C}$ are in $12.0 \mathrm{~g}$ of ibuprofen?
d. How many moles of ibuprofen contain $1.22 \times 10^{23}$ atoms of C?

Susan Hallstrom

Numerade Educator

01:42

Problem 83

Balance each of the following by adding coefficients, and identify the type of reaction for each: (7.1,7.2)

David Collins

Numerade Educator

01:07

Problem 84

Balance each of the following by adding coefficients, and identify the type of reaction for each: (7.1,7.2)

David Collins

Numerade Educator

Problem 85

If red spheres represent oxygen atoms, blue spheres represent sulfur atoms, and all the molecules are gases, (7.1,7.2)
a. write the formula for each of the reactants and products.
b. write a balanced equation for the reaction.
c. indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

David Collins

Numerade Educator

01:37

Problem 86

If purple spheres represent iodine atoms, white spheres represent chlorine atoms, the reacting molecules are solid, and the products are gases, (7.1,7.2)
a. write the formula for each of the reactants and products.
b. write a balanced equation for the reaction.
c. indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

David Collins

Numerade Educator

01:51

Problem 87

If blue spheres represent nitrogen atoms, purple spheres represent bromine atoms, and all the molecules are gases, (7.1,7.2)
a. write the formula for each of the reactants and products.
b. write a balanced equation for the reaction.
c. indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

David Collins

Numerade Educator

01:50

Problem 88

If green spheres represent chlorine atoms, yellow-green spheres represent fluorine atoms, white spheres represent hydrogen atoms, and all the molecules are gases, (7.4,7.5)
a. write the formula for each of the reactants and products.
b. write a balanced equation for the reaction.
c. indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

David Collins

Numerade Educator

Problem 89

If green spheres represent chlorine atoms, red spheres represent oxygen atoms, and all the molecules are gases, (7.4,7.5)
a. write the formula for each of the reactants and products.
b. write a balanced equation for the reaction.
c. indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

David Collins

Numerade Educator

Problem 90

If blue spheres represent nitrogen atoms, purple spheres represent iodine atoms, the reacting molecules are gases, and the products are solid, (7.4,7.5)
a. write the formula for each of the reactants and products.
b. write a balanced equation for the reaction.
c. indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

David Collins

Numerade Educator

05:50

Problem 91

Calculate the molar mass for each of the following: (7.2)
a. $\mathrm{CaSO}_{4}$
b. $\mathrm{H}_{2} \mathrm{SO}_{4}$
c. $\mathrm{NaCl}$
d. $\mathrm{C}_{6} \mathrm{H}_{6} \mathrm{O}$

Madeleine Sarner

Numerade Educator

Problem 92

Calculate the molar mass for each of the following: (7.5)
a. $\mathrm{C}_{8} \mathrm{H}_{10} \mathrm{~N}_{4} \mathrm{O}_{2},$ caffeine, found in coffee beans
b. $\mathrm{TiO}_{2}$, titanium dioxide, used in sunscreen lotion
c. $\mathrm{Al}(\mathrm{OH})_{3}$, aluminum hydroxide, used to relieve heartburn and upset stomach
d. $\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2},$ calcium phosphate, used to prevent and treat calcium deficiency

David Collins

Numerade Educator

Problem 93

How many grams are in 0.250 mole of each of the following? (7.5)
a. Ca
b. $\mathrm{O}_{2}$
c. $\mathrm{NaCl}$

David Collins

Numerade Educator

03:10

Problem 94

How many grams are in 1.750 moles of each of the following? (7.5)
a. $\mathrm{BeCl}_{2}$
b. $\mathrm{CaSO}_{4}$
c. $\mathrm{AlCl}_{3}$

Isaac Huidobro

Numerade Educator

01:42

Problem 95

How many moles of $\mathrm{O}$ are in $25.0 \mathrm{~g}$ of each of the following compounds? (7.2)
a. $\mathrm{CO}_{2}$
b. $\mathrm{Al}_{2} \mathrm{O}_{3}$
c. $\mathrm{NiCl}_{2} .6 \mathrm{H}_{2} \mathrm{O}$

David Collins

Numerade Educator

01:10

Problem 96

How many moles are in $6.0 \mathrm{~g}$ of each of the following compounds? (7.5)
a. $\mathrm{NO}_{2}$
b. $\mathrm{Na}_{2} \mathrm{CO}_{3}$
c. $\mathrm{HCl}$

David Collins

Numerade Educator

Problem 97

Identify the type of reaction for each of the following as combination, decomposition, single replacement, double replacement, or combustion: (7.3)
a. Potassium reacts with chlorine gas to form potassium chloride.
b. Potassium metal and chlorine gas are obtained from electrolysis of molten potassium chloride.
c. Heating starch in oxygen produces carbon dioxide and water.

David Collins

Numerade Educator

01:34

Problem 98

Identify the type of reaction for each of the following as combination, decomposition, single replacement, double replacement, or combustion: (7.5)
a. A compound breaks apart into its elements.
b. Copper and bromine form copper(II) bromide.
c. Iron(II) sulfite breaks down to iron(II) oxide and sulfur dioxide.
d. Silver ion from $\mathrm{AgNO}_{3}(a q)$ forms a solid with bromide ion from $\operatorname{KBr}(a q)$

David Collins

Numerade Educator

02:23

Problem 99

Balance each of the following chemical equations, and identify the type of reaction: (7.4,7.5)
a. $\mathrm{MgCO}_{3}(s) \longrightarrow \mathrm{MgO}(s)+\mathrm{CO}_{2}(g)$
b. $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)$
c. $\mathrm{Al}(s)+\mathrm{CuCl}_{2}(a q) \longrightarrow \mathrm{AlCl}_{3}(a q)+\mathrm{Cu}(s)$
d. $\operatorname{AgNO}_{3}(a q)+\mathrm{MgCl}_{2}(a q) \longrightarrow \mathrm{AgCl}_{2}(s)+\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}(a q)$

David Collins

Numerade Educator

02:30

Problem 100

Balance each of the following chemical equations, and identify the type of reaction: (8.1,8.2,8.3)
a. $\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{3}(a q)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{BaSO}_{4}(s)+\mathrm{HNO}_{3}(a q)$
b. $\mathrm{KCN}(a q)+\mathrm{H}_{3} \mathrm{PO}_{4}(a q) \longrightarrow \mathrm{HCN}(a q)+\mathrm{K}_{3} \mathrm{PO}_{4}(a q)$
c. $\mathrm{PbCl}_{2}(a q)+\mathrm{Al}(s) \longrightarrow \mathrm{AlCl}_{3}(a q)+\mathrm{Pb}(s)$
d. $\mathrm{C}_{2} \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)$

David Collins

Numerade Educator

01:08

Problem 101

Identify each of the following as an oxidation or a reduction: (7.6)
a. $\mathrm{Zn}^{2+}(a q)+2 e^{-} \longrightarrow \mathrm{Zn}(s)$
b. $\mathrm{Al}(s) \longrightarrow \mathrm{Al}^{3+}(a q)+3 e^{-}$
c. $\mathrm{Pb}(s) \longrightarrow \mathrm{Pb}^{2+}(a q)+2 e^{-}$
d. $\mathrm{Cl}_{2}(g)+2 e^{-} \longrightarrow 2 \mathrm{Cl}^{-}(a q)$

David Collins

Numerade Educator

01:06

Problem 102

Identify each of the following as an oxidation or a reduction: (7.6)
a. $\mathrm{Mg}^{2+}(a q)+2 e^{-} \longrightarrow \mathrm{Mg}(s)$
b. $2 \mathrm{I}^{-}(a q) \longrightarrow \mathrm{I}_{2}(s)+2 e^{-}$
c. $\mathrm{Li}(s) \longrightarrow \mathrm{Li}^{+}(a q)+e^{-}$
d. $\mathrm{Co}^{2+}(a q)+2 e^{-} \longrightarrow \mathrm{Co}(s)$

David Collins

Numerade Educator

05:14

Problem 103

When ammonia (NH $_{3}$ ) gas reacts with fluorine gas, the gaseous products are dinitrogen tetrafluoride $\left(\mathrm{N}_{2} \mathrm{~F}_{4}\right)$ and hydrogen fluoride $(\mathrm{HF}) .(7.4,7.7,7.8)$
a. Write the balanced chemical equation.
b. How many moles of each reactant are needed to produce 4.00 moles of HF?
c. How many grams of $\mathrm{F}_{2}$ are needed to react with $25.5 \mathrm{~g}$ of $\mathrm{NH}_{3} ?$
d. How many grams of $\mathrm{N}_{2} \mathrm{~F}_{4}$ can be produced when $3.40 \mathrm{~g}$ of $\mathrm{NH}_{3}$ reacts?

David Collins

Numerade Educator

05:05

Problem 104

When nitrogen dioxide $\left(\mathrm{NO}_{2}\right)$ gas from car exhaust combines with water vapor in the air, it forms aqueous nitric acid (HNO $_{3}$ ), which causes acid rain, and nitrogen oxide gas. (7.4,7.7,7.8)
a. Write the balanced chemical equation.
b. How many moles of each product are produced from 0.250 mole of $\mathrm{H}_{2} \mathrm{O} ?$
c. How many grams of $\mathrm{HNO}_{3}$ are produced when $60.0 \mathrm{~g}$ of $\mathrm{NO}_{2}$ completely reacts?
d. How many grams of $\mathrm{NO}_{2}$ are needed to form $75.0 \mathrm{~g}$ of $\mathrm{HNO}_{3}$ ?

David Collins

Numerade Educator

01:43

Problem 105

Pentane gas, $\mathrm{C}_{5} \mathrm{H}_{12}$, undergoes combustion with oxygen gas to produce carbon dioxide and water gases. (7.4,7.8)
a. Write the balanced chemical equation.
b. How many grams of $\mathrm{C}_{5} \mathrm{H}_{12}$ are needed to produce $72 \mathrm{~g}$ of water?
c. How many grams of $\mathrm{CO}_{2}$ are produced from $32.0 \mathrm{~g}$ of $\mathrm{O}_{2} ?$

David Collins

Numerade Educator

01:39

Problem 106

Propane gas, $\mathrm{C}_{3} \mathrm{H}_{8}$, undergoes combustion with oxygen gas to produce carbon dioxide and water gases. Propane has a density of $2.02 \mathrm{~g} / \mathrm{L}$ at room temperature. (7.4,7.8)
a. Write the balanced chemical equation.
b. How many grams of $\mathrm{H}_{2} \mathrm{O}$ form when $5.00 \mathrm{~L}$ of $\mathrm{C}_{3} \mathrm{H}_{8}$ reacts?
c. How many grams of $\mathrm{H}_{2} \mathrm{O}$ can be produced from the reaction of $100 . \mathrm{g}$ of $\mathrm{C}_{3} \mathrm{H}_{8} ?$

David Collins

Numerade Educator

Problem 107

The equation for the formation of silicon tetrachloride from silicon and chlorine is (7.9)
$$
\mathrm{Si}(s)+2 \mathrm{Cl}_{2}(g) \longrightarrow \mathrm{SiCl}_{4}(g)+157 \mathrm{kcal}
$$
a. Is the formation of $\mathrm{SiCl}_{4}$ an endothermic or exothermic reaction?
b. Is the energy of the product higher or lower than the energy of the reactants?

David Collins

Numerade Educator