1. Kc for a reaction is 160. Solve for the value of Kp for the following reaction
at 30°C.
A (g) + 2 B (g) ---> C (g)
2. The equilibrium pressures for N2 and H2 respectively are as follows 0.928
and 0.432. If Kp = 1.45 x 10-5 at 500°C what is the partial pressure of
NH3?
N2 (g) + 3 H2 (g) <===> 2 NH3 (g)
3. Write the equilibrium expression for the reaction:
SnO2 (s) + 2 CO (g) <---> Sn(s) + 2 CO2 (g)
What is the value of Kc if the concentrations are all tripled?
4. A gas vessel is charged with a mixture of PCl3 and Cl2 and allowed to equilibrate at 450 K. At
equilibrium the partial pressures of the three gases are PPCl3 = 0.124, PCl2 = 0.157, and PPCl5 =
1.30 atm. What is the value of Kp.
5. Consider the reaction:
2 SO2 (g) + O2 (g) <==> 2 SO3 (g)
Which direction would the following changes make the reaction shift:
a. PT decrease
b. PSO2 increase
c. Adding a catalyst
6. Find the rate equation including k for the reaction:
2 NO (g) + O2 (g) ---> 2 NO2 given the following data.
[NO] M [O2]M Initial Rate (M/s)
0.0126 0.0125 0.0141
0.0252 0.0250 0.113
0.0252 0.0125 0.0564
7. The thermal decomposition of N2O5 (g) to form NO2 (g) and O2 (g) is a first-order reaction.
The rate constant for the reaction is 5.1 x 10-4 s at 318 K.
a. What is the half-life for this process.
b. If the initial concentration of N2O5 (g) is 0.250 M, what is the concentration after 10 seconds?
8. The activation energy for a process is 76.7 kJ/mol. How many times faster will the reaction
occur at 50°C than at 0°C.
9. The reaction listed below is a second order process. Find the concentration after 5.00 minutes
if k=1.25 x 10-2M-1min-1 and the initial concentration of A is 0.0125M
A + 2 B -----> C
10. What are the units of k for the following reaction?
Rate = k [A][B]-2 [C]0