Q: Which equation correctly relates the total pressure in a mixture of air and an evaporated volatile liquid?

$$P_{\text{total}} = P_{\text{air}} + P_{\text{vapor}}$$

Question 1

A volatile liquid fully evaporates inside a closet with a volume of $$2.2\ \mathrm{m}^3$$, displacing air. If the closet initially contains air at $$1.2\ \mathrm{atm}$$, composed of $$20.0\%$$ $$\mathrm{O}_2$$ and $$80.0\%$$ $$\mathrm{N}_2$$, what is the partial pressure of $$\mathrm{O}_2$$ remaining after $$32\% of $$the air is displaced by the vapor?

Accepted Answer

$$P_{O_2$} = 0.163\ \mathrm{atm}$$

Question 2

Which equation correctly relates the total pressure in a mixture of air and an evaporated volatile liquid?

Accepted Answer

$$P_{	ext{total}} = P_{	ext{air}} + P_{	ext{vapor}}$$

Question 3

A closet contains air at $$1.2\ \mathrm{atm}$$, with $$80\%$$ $$\mathrm{N}_2$$ and $$20\%$$ $$\mathrm{O}_2. If$$ $$32\% of $$the air is displaced by a vapor, what is the partial pressure of $$\mathrm{N}_2$$ remaining?

Accepted Answer

$$P_{N_2$} = 0.653\ \mathrm{atm}$$

Question 4

If the mass density of humid air is $$6\%$$ less than dry air at the same temperature and pressure, which of the following best explains this phenomenon?

Accepted Answer

Water vapor has a lower molar mass than $$\mathrm{N}_2$$ and $$\mathrm{O}_2$$, so replacing air molecules with $$\mathrm{H}_2\mathrm{O}$$ decreases the mass per unit volume.

Question 5

A solution contains $$0.100\ \mathrm{L} of$$ $$1.22\ \mathrm{M}$$ $$\mathrm{NaI}. $$How many moles of $$\mathrm{NaI}$$ are present?

Accepted Answer

$$0.122\ \mathrm{mol}$$

Question 6

Given the reaction $$\mathrm{Ag}^+(aq) + \mathrm{NaI}(aq) \rightarrow \mathrm{AgI}(s) + \mathrm{Na}^+(aq)$$, what is the limiting reactant if $$0.122\ \mathrm{mol}$$ $$\mathrm{NaI}$$ and $$0.100\ \mathrm{mol}$$ $$\mathrm{Ag}^+$$ are mixed?

Accepted Answer

$$\mathrm{Ag}^+$$

Question 7

In the reaction $$\mathrm{Hg}^{2+}(aq) + 2\mathrm{NaI}(aq) \rightarrow \mathrm{HgI}_2(s) + 2\mathrm{Na}^+(aq)$$, how many moles of $$\mathrm{NaI}$$ are required to completely react with $$0.050\ \mathrm{mol} of$$ $$\mathrm{Hg}^{2+}$$?

Accepted Answer

$$0.100\ \mathrm{mol}$$

Question 8

A $$5\ \mathrm{L}$$ rigid container at $$225\ \mathrm{K}$$ contains $$15.0\ \mathrm{g} of$$ $$\mathrm{O}_3$$ and $$25.0\ \mathrm{mmHg} of$$ $$\mathrm{CF}_3\mathrm{Cl}. $$After the reaction $$\mathrm{CF}_3\mathrm{Cl}(g) + 2\mathrm{O}_3(g) \rightarrow \mathrm{Cl}(g) + 3\mathrm{O}_2(g) + \mathrm{CF}_3(g)$$, what is the final pressure of $$\mathrm{O}_2$$?

Accepted Answer

$$0.0454\ \mathrm{atm}$$

Question 9

What is the molar mass of $$\mathrm{CF}_3\mathrm{Cl}$$ used in the gas reaction calculations?

Accepted Answer

$$104.46\ \mathrm{g/mol}$$

Question 10

A metal oxide has the empirical formula $$\mathrm{MO}. If $$the oxide contains $$20.0\%$$ oxygen by mass, what is the identity of the metal?

Accepted Answer

Magnesium ($$\mathrm{Mg})$$

Question 11

Which of the following best describes the role of stoichiometry in determining the mass of precipitate formed in a reaction?

Accepted Answer

Stoichiometry allows calculation of the amount of product formed from known reactant quantities using mole ratios.

Question 12

If $$0.122\ \mathrm{mol}$$ $$\mathrm{NaI} is $$added to a solution containing $$\mathrm{Ag}^+$$, what mass of $$\mathrm{AgI}$$ will precipitate? ($$M_{\mathrm{AgI}} = 234.77\ \mathrm{g/mol})$$

Accepted Answer

$$28.7\ \mathrm{g}$$

Question 13

Which gas law is most appropriate for calculating the pressure of a gas in a rigid container at constant temperature?

Accepted Answer

$$P = \frac{nRT}{V}$$

Question 14

In the reaction $$\mathrm{CF}_3\mathrm{Cl}(g) + 2\mathrm{O}_3(g) \rightarrow \mathrm{Cl}(g) + 3\mathrm{O}_2(g) + \mathrm{CF}_3(g)$$, what is the mole ratio of $$\mathrm{O}_3$$ consumed to $$\mathrm{O}_2$$ produced?

Accepted Answer

$$2:3$$

Question 15

A closet contains air at $$1.2\ \mathrm{atm}$$, and $$32\% of $$the air is replaced by a vapor. What is the partial pressure of the vapor?

Accepted Answer

$$0.384\ \mathrm{atm}$$

Question 16

Which of the following is a correct application of Dalton's Law of Partial Pressures?

Accepted Answer

The total pressure of a mixture of gases is the sum of the partial pressures of each individual gas.

Question 17

If $$0.02465$$ moles of $$\mathrm{O}_3$$ remain after a reaction in a $$5\ \mathrm{L}$$ container at $$225\ \mathrm{K}$$, what is the pressure of $$\mathrm{O}_3$$? ($$R = 0.08206\ \mathrm{L\ atm\ $$mol^{-1}$$\ K$$^{-1}$$})$$

Accepted Answer

$$0.090\ \mathrm{atm}$$

General Chemistry Principles I: Gases, Stoichiometry, and Energetics (Fall 2025 Study Notes)

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