1. A gas is held in a glass container with an open-tube manometer and a thermometer attached to it. The
pressure is 755 torr and the temperature is 25 °C. If the gas is cooled at constant pressure to a volume
that is one-half it initial volume, what is the final temperature?
2. A certain second-order decomposition reaction has a rate constant equal to 0.0023 L/mol·sec. If the
initial concentration of the reactant is 5.0 M, what is the reactant concentration after 12 seconds?
3. The pH of a 0.250 M unknown weak acid solution is measured to be 3.40. What is the Ka for this weak
acid?
4. Consider the following reaction and stated equilibrium constant:
Xe(g) + 2 F2(g) ↔ XeF4(g) Kp = 0.0025 atm-2
If we introduce 0.50 atm of Xe and 0.50 atm of F2 into an empty flask, what will be the partial pressure
of all three gases in the mixture at equilibrium?
5. Calculate the pH of a solution prepared by adding 21.00 mL of 0.300 M sodium hydroxide to
25.00 mL of 0.400 M benzoic acid.
6. What is the pH of a buffer solution formed by mixing 47.00 mL of a 5.250 M sodium acetate solution
with 53.00 mL of a 4.750 M acetic acid solution?
7. A certain decomposition reaction follows first-order kinetics. If the time it takes for half the reactant to
decompose is 12.0 hours, what is the rate constant for the reaction?
8. The specific heat capacity of water is 4.184 J/g·K. Suppose 1.50 grams of water are placed in a
calorimeter at 25 °C. How much energy, in the form of heat, would be needed to raise the temperature
of the water to 100 °C?
9. Consider the following reaction between propane and oxygen gas:
C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g)
What is the density of the carbon dioxide produced if 0.540 atm of oxygen reacts with excess propane
in 2.00 L steel vessel at 423 K.
10. Use the changes in enthalpy, entropy and free energy to calculate the equilibrium constant of the
following reaction at 115 °C.
PCl5(g) ↔ PCl3(g) + Cl2(g)
11. What is the pOH of a solution of 0.116-M sodium acetate (NaCH3COO)?
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