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ch 13 part of 15 review ws
1] At 500 oC, K = 6.0 x 10-2 L/n for the equilibrium: 3H2(g) + N2(g) ↔ 2NH3(g).
Find the equilibrium concentration of hydrogen if the equilibrium concentration of the
nitrogen is 0.921 M and the equilibrium concentration of the ammonia is 0.157 M.
0.76 M
2] Consider the equilibrium: 4HCl(g) + O2(g) ↔ 2H2O(g) + 2Cl2(g)
K = 1.6 L/n at 27oC. Find a] Kp
b] the direction of the equilibrium shift if I start with:
i] PHCl = PO2 = PH2O = 0.20 atm; PCl2 = 1.7 x 10-4 atm
ii] PHCl = 0.30 atm; PO2 = 0.15 atm; PH2O = 0.35 atm; PCl2 = 0.20 atm
iii] PHCl = PCl2 = PH2O = 1.75 atm; PO2 = 15.4 atm
A] 0.065 Bi] right ii] left iii] at equilibrium
3] For the system: 2HI(g) ↔ H2(g) + I2(g); K = 0.016 at 800 K. If the pressure of the HI is
initially 0.50 atm, find the equilibrium pressures of all species.
[H2] = [I2] = 0.050 atm; [HI] = 0.40 atm
4] At some temperature, K =1.5 x 10-7 for the equilibrium reaction:
2CO2(g) ↔ 2CO(g) + O2(g). If 4.0 mol of CO2 is placed in a 2.0 L container, calculate the
equilibrium concentrations of all species.
[O2] = 5.3 x 10-3 M; [CO] = 1.1 x 10-2 M; [CO2] = 2.0 M
5] Consider the equilibrium system: 4NH3(g) + 3O2(g) ↔ 2N2(g) + 6H2O(l)
∆H = -1530.4 kj/mol. How will the amount of ammonia be affected by
a] removing oxygen gas ↑
b] adding nitrogen gas ↑
c] adding water no ∆
d] expanding the container ↑
f] increasing the temperature ↑
e] decreasing the pressure by changing the volume ↑
g] adding a catalyst no ∆
h] adding neon gas no ∆
6] At 0oC, K = 22 for an equilibrium reaction. If K = 49 at 27oC, is the reaction
exothermic or endothermic? endothermic
7] Given the following equilibrium constants for two imaginary reactions:
A(g) + T(g) ↔ Q(g) + R(g) ;
K = 5.0
R(g) + A(g) ↔ T(g) + L(g) ;
K = 0.75
Find the value of the equilibrium constant for:
A] Q(g) + L(g) ↔ 2A 0.27
B] A(g) ↔ ½ Q(g) + ½ L(g)
1.9
8] Given the equilibrium reaction:
2 AsH3(g) ↔ 2 As(s) + 3 H2(g)
If pure AsH3 is put into a rigid, sealed 1.00 L flask at 400. torr at 25.0oC, and after
equilibrium is attained, the final total pressure is 492 torr, find
A] the equilibrium partial pressures of AsH3 and the H2 [AsH3] = .284 atm; [H2] = 0.363
atm
B] the mass in grams of the arsenic that is produced 0.741 g
C] calculate Kp 0.593 atm
9] Find the solubility of:
A] AgBr 7.1 x 10-7 M
B] PbCl2 1.6 x 10-2 M
C] Ag3PO4
1.6 x 10-5 M
10] Given that the solubility of Ag2C2O4, silver oxalate, is 1.1 x 10-4, find the Ksp for
silver oxalate 5.3 x 10-12
11] Will a precipitate form if I mix 25.0 mL of 0.060 M Pb(NO3)2 with 75.0 mL of
0.14 M NaI?
Q = 1.7 x 10-4 yes
12] Find the solubility of PbCl2 in
A] pure water1.6 x 10-2 M b] 0.10 M Pb(NO3)2 6.3 x 10-3 M c] 0.10 M NaCl 1.6 x 10-3 M
13] Which is less soluble?
A] AgOH or AgCl?
B] AgCl or CaF2
In both cases, the AgCl is less soluble