Q: A 5.0-L tank contains helium gas at 1.50 atm. What is the pressure of the gas in mmHg?

$$1.50 \times 760 = 1140$$ mmHg

Q: Consider the balanced equation: $$KCl(aq) + $$AgNO_3$$(aq) \rightarrow $$KNO_3$$(aq) + AgCl(s). $$How many mL of 0.234 M KCl solution will react completely with 25.0 mL of 0.161 M AgNO$$_3$$ solution?

$$25.0 \times 0.161 / 0.234 = 17.2 mL$$

Q: At STP conditions of T and P, what is the mass of 11.2 liters of O$$_2$$ gas?

$$11.2 \text{ L} \times \frac{32 \text{ g}}{22.4 \text{ L}} = 16 \text{ g}$$

Q: A gas contained in a steel tank has a pressure of 1.3 atm at a temperature of 320K. What will be the pressure if the temperature drops to 280K?

$$P_2$$ = $$P_1$$ \times \frac{$$T_2$$}{$$T_1$$} = 1.3 \times \frac{280}{320} = 1.14$$ atm

Question 1

A 5.0-L tank contains helium gas at 1.50 atm. What is the pressure of the gas in mmHg?

Accepted Answer

$$1.50 	imes 760 = 1140$$ mmHg

Question 2

Which statement best describes the vapor pressure of a liquid?

Accepted Answer

It increases as the temperature of the liquid increases.

Question 3

Consider the balanced equation: $$KCl(aq) + $$AgNO_3$$(aq) \rightarrow $$KNO_3$$(aq) + AgCl(s). $$How many mL of 0.234 M KCl solution will react completely with 25.0 mL of 0.161 M AgNO$$_3$$ solution?

Accepted Answer

$$25.0 	imes 0.161 / 0.234 = 17.2 mL$$

Question 4

At 40°C, approximately 130 g of KI are added to 100 g of water. The solution formed is:

Accepted Answer

Unsaturated

Question 5

At STP conditions of T and P, what is the mass of 11.2 liters of O$$_2$$ gas?

Accepted Answer

$$11.2 	ext{ L} 	imes \frac{32 	ext{ g}}{22.4 	ext{ L}} = 16 	ext{ g}$$

Question 6

Aqueous hydrofluoric acid (HF(aq)) is a weak acid. Which statement is TRUE about HF(aq) in water?

Accepted Answer

HF(aq) only partially ionizes in water, producing small amounts of H$$_3O$^+$$ and F$$^-.$$

Question 7

A gas contained in a steel tank has a pressure of 1.3 atm at a temperature of 320K. What will be the pressure if the temperature drops to 280K?

Accepted Answer

$$P_2$$ = $$P_1$$ 	imes \frac{$$T_2$$}{$$T_1$$} = 1.3 	imes \frac{280}{320} = 1.14$$ atm

Question 8

When aqueous solutions of NH$$_4Cl $$and KNO$$_3$$ are mixed, what forms?

Accepted Answer

No precipitate forms; NH$$_4NO$_3$$ and KCl remain in solution

Question 9

In the kinetic molecular theory of gas behavior, the assumption is made that gas molecules:

Accepted Answer

Move rapidly in random directions

Question 10

Which diagram best represents a reversible reaction that has reached equilibrium?

Accepted Answer

Diagram C

Question 11

Carbon dioxide will form when carbon monoxide reacts with molecular oxygen according to the balanced chemical equation: $$2CO(g) + O_2$(g) \rightarrow 2CO_2(g). If a $$mixture of CO and O$$_2$$ are put into a container, which reactant is the limiting reactant and how much reactant is left in the container when the reaction is finished?

Accepted Answer

CO is the limiting reactant. There are 2 molecules of O$$_2$$ left in the container.

Question 12

What is the molarity of a solution that contains 3.25 moles of KNO$$_3 in 250 mL of $$solution, assuming the solution is unsaturated?

Accepted Answer

$$M = \frac{3.25}{0.250} = 13.0 M$$

Question 13

Given the balanced equation: $$TiCl_4(aq) + 2$$NaOH(aq) \rightarrow TiO_2H_2O(s) + 4NaCl(aq)$$, which of the following is the correct net ionic equation?

Accepted Answer

$$Ti^{4+}(aq) + 2OH^-(aq$$) \rightarrow TiO_2H_2O(s)$$

Question 14

A steel tank contains a mixture of helium, neon, and argon gases. If the total pressure in the tank is 492 mmHg, and the partial pressures of helium and argon are 119 mmHg and 116 mmHg, respectively, what is the partial pressure of neon?

Accepted Answer

$$492 - (119 + 116) = 257$$ mmHg

Question 15

Consider the reversible reaction: $$2NO_2(g) \rightleftharpoons 2NO(g) + O_2$(g). $$Which statement is TRUE regarding this reaction?

Accepted Answer

At equilibrium, the forward and reverse reactions occur at the same rate.

Question 16

A patient needs to receive 85 grams of glucose every 12 hours. What volume of a 5.5% (m/v) aqueous glucose solution needs to be administered to the patient each 12-hour period?

Accepted Answer

$$\frac{85}{0.055} = 1545 mL$$

Question 17

Air bags in vehicles inflate when the following reaction occurs: $$2NaN_3(s) \rightarrow 2Na(s) + 3N_2(g). $$What mass, in grams, of NaN$$_3 is $$required to produce 3.00 L of N$$_2$$ gas at STP conditions?

Accepted Answer

$$3.00 	ext{ L} 	imes \frac{1 	ext{ mol}}{22.4 	ext{ L}} 	imes \frac{2 	ext{ mol NaN}_3}{3 	ext{ mol N}_2} 	imes 65.01 	ext{ g/mol} = 11.6 	ext{ g}$$

Question 18

If white blood cells (leukocytes) are isolated from the blood and then placed into a hypotonic solution, what would happen?

Accepted Answer

The cells would expand in volume.

Question 19

Water is a polar solvent and hexane (C$$_6H$_{14}) is a $$nonpolar solvent. Which of the following correctly describes the solubility of each of the following solutes?

Accepted Answer

NaCl is soluble in water; mineral oil is soluble in hexane.

General Chemistry I: Exam Study Guide (GOB Chemistry Topics)

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