When the gases dihydrogen sulfide and oxygen react, they...

When the gases dihydrogen sulfide and oxygen react, they form the gases sulfur dioxide and water vapor. a. Write the balanced chemical equation for the reaction. b. How many grams of oxygen are required to react with $2.50 \mathrm{~g}$ of dihydrogen sulfide? c. How many grams of sulfur dioxide can be produced when $38.5 \mathrm{~g}$ of oxygen reacts? d. How many grams of oxygen are required to produce $55.8 \mathrm{~g}$ of water vapor?

When the gases dihydrogen sulfide and oxygen react, they form the gases sulfur dioxide and water vapor.
a. Write the balanced chemical equation for the reaction.
b. How many grams of oxygen are required to react with $2.50 \mathrm{~g}$ of dihydrogen sulfide?
c. How many grams of sulfur dioxide can be produced when $38.5 \mathrm{~g}$ of oxygen reacts?
d. How many grams of oxygen are required to produce $55.8 \mathrm{~g}$ of water vapor?

Key Concepts

Chemical Reaction Balancing

Balancing chemical reactions involves ensuring that the number of atoms of each element is equal on both sides of the equation. This principle is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. Achieving a balanced equation is essential for performing any quantitative analysis in chemistry, such as calculating the amounts of reactants required or the products formed.

Stoichiometry

Stoichiometry is the study of the quantitative relationships between the amounts of reactants and products in a chemical reaction. It uses the coefficients from the balanced chemical equation to establish mole ratios that allow the conversion between reactant amounts and product amounts. This concept is foundational when determining the mass of a substance required or produced in a reaction.

Mole Concept

The mole concept is a central idea in chemistry which defines a mole as a specific number of entities (Avogadro's number, approximately 6.022 x 10^23). It provides a bridge between the microscopic scale of atoms and molecules and the macroscopic scale of grams and liters, allowing chemists to count particles by weighing samples. This concept is critical when converting grams to moles and vice versa during reaction calculations.

Molar Mass Calculations

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole. It is calculated by summing the atomic masses of all atoms in a molecule as found on the periodic table. Molar mass serves as a conversion factor in stoichiometric calculations, enabling the conversion between the mass of a substance and the number of moles to facilitate quantitative analysis in chemical reactions.

Transcript

00:01 We are told that the gas is dihydrogen sulfide, which i've written right here, and oxygen react.

00:08 They form the gases sulfur dioxide and water vapor.

00:21 Our first order of business is to write the balanced chemical equation.

00:27 I guess i need a two here, two here, two here, and a three here.

00:36 This is a little bit nicer.

00:40 So i have four hydrogens, four hydrogens.

00:43 Two sulfurs, two sulfurs.

00:45 Six oxygens and four, five, six oxygen.

00:48 Now we have three calculations that we're asked to perform.

00:56 We are given 22 .50 grams of dihydrogen sulfide and we're asked to convert that to grams of oxygen.

01:11 That'll be a simple stoichiometric calculation.

01:16 We'll start with our 2 .50 grams of hydrogen sulfide, which we will convert to moles using the molar mass of h2s.

01:33 I usually just type things into my computer, phone, whatever.

01:47 So that's my molar mass of h2s.

01:49 Now i'm going to use my mole ratios for my balanced chemical equation for h2s, which has a coefficient of 2, and o2, which has a coefficient of 3.

02:01 Finally, my last step will be 32 grams of oxygen per mole of oxygen, which is the molar mass of oxygen.

02:11 So i'll take 2 .5 times 3 times.

02:14 32.

02:23 So i got 3 .52 grams of oxygen.

02:32 Let's make that a nicer 3.

02:39 B.

02:44 Question b...

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