Raising the temperature of the reaction mixture will:

Raising the temperature of the reaction mixture will:

a. cause [CO2] to increase c. have no effect
b. cause [H2O] to increase d. cannot be determined


Answer: b. cause [H2O] to increase

Addition of CO to an equilibrium mixture of the above reaction will

Addition of CO to an equilibrium mixture of the above reaction will

a. cause [CO2] to increase c. have no effect
b. cause [H2O] to increase d. cannot be determined


Answer: a. cause [CO2] to increase

If you mixed 5.0 mol CO2, 0.10 mol H2, 3.5 mol of CO, and 0.0010 mol H2O in a one-liter container, in which direction would the reaction proceed?

If you mixed 5.0 mol CO2, 0.10 mol H2, 3.5 mol of CO, and 0.0010 mol H2O in a one-liter container, in which direction would the reaction proceed?

a. To the left.
b. To the right.
c. The above mixture is the equilibrium mixture.
d. Cannot tell from the information given.


Answer: b. To the right.

The equilibrium constant, Kc, for the following reaction is 1.20 x 10-2 at 500K: PCl5(g) PCl3(g) + Cl2(g). Calculate Kp for this reaction.

The equilibrium constant, Kc, for the following reaction is 1.20 x 10-2 at 500K: PCl5(g) PCl3(g) + Cl2(g). Calculate Kp for this reaction.

a. 0.0120
b. 0.492
c. 49.9
d. 20.2
e. 7.13 x 10-6


Answer: b. 0.492

If an equilibrium mixture of the three gases in a 5.0L container at 298K contains 0.304mol of NOBr gas and 0.401mol of Br2 gas, what is the equilibrium concentration of NO?

The equilibrium constant, K, for the following reaction is 6.50 x 10-3 at 298K

2NOBr(g) 2NO(g) + Br2(g)

If an equilibrium mixture of the three gases in a 5.0L container at 298K contains 0.304mol of NOBr gas and 0.401mol of Br2 gas, what is the equilibrium concentration of NO?

a. 6.14 x 10^-2 M
b. 3.74 x 10^-3 M
c. 4.93 x 10^-3 M
d. 1.73 x 10^-2 M
e. 3.00 x 10^-4 M


Answer: d. 1.73 x 10^-2 M

Which of the following statements is true about the above reaction?

The equilibrium constant, K, for the following reaction is 1.96 x 105 at 548K

NH3(g) + HCl(g) NH4Cl (s)

Which of the following statements is true about the above reaction?

a. The reaction favors the products and the concentrations of NH3 and HCl will be low at equilibrium.
b. The reaction favors the reactants and the concentrations of NH3 and HCl will be high at equilibrium
c. The reaction favors the product and the equilibrium concentration of NH4Cl equals 1.
d. The reaction favors the reactants and the equilibrium concentration of NH4Cl equals 1.
e. Two of the above are true.


Answer: a. The reaction favors the products and the concentrations of NH3 and HCl will be low at equilibrium.