Question 1

What is stoichiometry?

Accepted Answer

The relationship between moles of each substance in a reaction.

Answer

The relationship between the periodic table and the molar mass.

Answer

The relationships between moles of reactants and mass of products.

Answer

The quantitative relationships between amounts of reactants used and products formed by a chemical reaction.

Question 2

In order to perform stoichiometric calculations, you must have _____.

Accepted Answer

a balanced chemical equation

Answer

the mass of each product

Answer

the mass of each reactant

Answer

a skeleton equation

Question 3

The coefficients in a balanced chemical reaction indicate ____.

Accepted Answer

the number of moles of each substance in the chemical reaction

Answer

the molar mass of each substance in the chemical reaction

Answer

the mass of each reactant and product in the chemical reaction

Answer

the percent composition of each element

Question 4

Mole ratios are obtained from ____.

Accepted Answer

balanced chemical equations

Answer

molar mass of the compounds

Answer

skeleton equations

Answer

periodic table

Question 5

Stoichiometry is based on what natural law?

Accepted Answer

law of conservation of mass

Answer

law of definite proportions

Answer

law of conservation of energy

Answer

law of multiple proportions

Question 6

What is the mole ratio between Nitrogen and Ammonia in the reaction shown below?

$\mathrm{N}_2+3\ \mathrm{H}_2\ \ \ \longrightarrow\ \ 2\ \mathrm{N}\mathrm{H}_3$

Accepted Answer

1:2

Answer

3:2

Answer

1:1

Answer

1:3

Question 7

What is the relationship between moles Mg to moles Fe in the balanced chemical equation below?

$\mathrm{N}_2+3\ \mathrm{H}_2\ \ \ \longrightarrow\ \ 2\ \mathrm{N}\mathrm{H}_3$

Accepted Answer

3 moles Mg = 2 moles Fe

Answer

3 moles MgO = 3 moles Fe

Answer

3 moles Mg = 1 mole Fe₂O₃

Answer

2 moles Mg = 3 moles Fe

Question 8

How many moles of water can be produced from 8 moles of H₂ in the reaction shown below?

$\mathrm{2\ H}_2+\mathrm{\mathrm{O}_2\ \ \longrightarrow\ \ 2\ \mathrm{H}_2\mathrm{O}}$

Accepted Answer

8 moles

Answer

2 moles

Answer

4 moles

Answer

1 mole

Question 9

Using the balanced chemical equation below, calculate the number of moles of oxygen gas needed to produce 20 moles of water.

$\mathrm{N}_2+3\ \mathrm{H}_2\ \ \ \longrightarrow\ \ 2\ \mathrm{N}\mathrm{H}_3$

Accepted Answer

34 moles O₂

Answer

20 moles O₂

Answer

24 moles O₂

Answer

8.5 moles O₂

Question 10

In a single displacement reaction, magnesium metal reacts with hydrochloric acid to produce magnesium chloride and hydrogen gas according to the balanced chemical equation shown below.

$\mathrm{N}_2+3\ \mathrm{H}_2\ \ \ \longrightarrow\ \ 2\ \mathrm{N}\mathrm{H}_3$

If you have 2.43 grams of Mg, what is the correct order of steps to convert from grams Mg to grams of HCl?

Accepted Answer

g Mg ⟶ moles Mg ⟶ moles HCl ⟶ g HCl

Answer

moles mg ⟶ g Mg ⟶ g HCl ⟶ moles HCl

Answer

moles Mg ⟶ moles HCl

Answer

g HCl ⟶ moles HCl ⟶ moles Mg ⟶ g Mg

Question 11

Ammonia reacts with oxygen gas to produce water and nitric oxide according to the balanced chemical equation below.

$\mathrm{N}_2+3\ \mathrm{H}_2\ \ \ \longrightarrow\ \ 2\ \mathrm{N}\mathrm{H}_3$

If you have $3.65 imes10^{23}$ molecules of NH₃, what is the correct order of steps to convert from molecules of NH₃ to liters of NO?

Accepted Answer

molecules NH₃ ⟶ moles NH₃ ⟶ moles NO ⟶ volume NO

Answer

g NH₃ ⟶ moles NH₃ ⟶ moles NO ⟶ g NO

Answer

moles NH₃ ⟶ moles NO ⟶ volume NO

Answer

moles NH₃ ⟶ molecules NH₃ ⟶ g NO ⟶ moles NO

Question 12

Using the balanced chemical equation below, calculate the number of moles of hexane (C₆H₁₀) needed to produce 305 g of water.

$2\mathrm{\ C}_6\mathrm{H}_{10}+17\ \mathrm{O}_2\ \ \longrightarrow\ \ 12\ \mathrm{\mathrm{C}O}_2+10\ \mathrm{H}_2\mathrm{O}$

Accepted Answer

3.39 moles C₆H₁₀

Answer

84.6 moles C₆H₁₀

Answer

278 moles C₆H₁₀

Answer

51.3 moles C₆H₁₀

Question 13

Using the balanced chemical equation below, if you burn 52 g of C₆H₁₀, what mass of CO₂ is released?

$2\mathrm{\ C}_6\mathrm{H}_{10}+17\ \mathrm{O}_2\ \ \longrightarrow\ \ 12\ \mathrm{\mathrm{C}O}_2+10\ \mathrm{H}_2\mathrm{O}$

Accepted Answer

167 g CO₂

Answer

47 g CO2

Answer

1.1 g CO₂

Answer

4.5 g CO₂

Question 14

For the balanced chemical reaction shown below, how many liters of H₂ are required at standard temperature and pressure to consume 45 liters of N₂?

$2\mathrm{\ C}_6\mathrm{H}_{10}+17\ \mathrm{O}_2\ \ \longrightarrow\ \ 12\ \mathrm{\mathrm{C}O}_2+10\ \mathrm{H}_2\mathrm{O}$

Accepted Answer

135 L H2

Answer

45 L H2

Answer

60 L H2

Answer

90 L H2

Question 15

For the balanced chemical reaction shown below, how many grams of H₂ are required at standard temperature and pressure to produce 30 liters of NH₃?

$2\mathrm{\ C}_6\mathrm{H}_{10}+17\ \mathrm{O}_2\ \ \longrightarrow\ \ 12\ \mathrm{\mathrm{C}O}_2+10\ \mathrm{H}_2\mathrm{O}$

Accepted Answer

4.05 g H₂

Answer

1.80 g H₂

Answer

2.03 g H₂

Answer

8.10 g H₂

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