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Problem 31b,c
Calculate Kc for each reaction.
b. CH4(g) + H2O(g) ⇌ CO(g) + 3 H2(g) Kp = 7.7x1024 (at 298 K)
c. I2(g) + Cl2(g) ⇌ 2 ICl(g) Kp = 81.9 (at 298 K)
Problem 32b,c
Calculate Kp for each reaction.
b. N2(g) + 3 H2(g) ⇌ 2 NH3(g) Kc = 3.7⨉108 (at 298 K)
c. N2(g) + O2(g) ⇌ 2 NO(g) Kc = 4.10⨉10-31 (at 298 K)
Problem 71a,b,d,f
Coal, which is primarily carbon, can be converted to natural gas, primarily CH4, by the exothermic reaction: C(s) + 2 H2(g) ⇌ CH4(g) Which disturbance will favor CH4 at equilibrium?
a. adding more C to the reaction mixture b. adding more H2 to the reaction mixture d. lowering the volume of the reaction mixture f. adding neon gas to the reaction mixture
- Nitrogen dioxide dimerizes according to the reaction: 2 NO2(g) ⇌ N2O4(g) Kp = 6.7 at 298 K. A 2.25-L container contains 0.055 mol of NO2 and 0.082 mol of N2O4 at 298 K. Is the reaction at equilibrium? If not, in which direction will the reaction proceed?
Problem 5
- Consider the reaction: CO(g) + H2O(g) ⇌ CO2(g) + H2(g) Kp = 0.0611 at 2000 K. A reaction mixture initially contains a CO partial pressure of 1344 torr and a H2O partial pressure of 1766 torr at 2000 K. Calculate the equilibrium partial pressures of each of the products.
Problem 6
- This reaction is exothermic. C6H12O6(s) + 6 O2(g) ⇌ 6 CO2(g) + 6 H2O(g). Predict the effect (shift right, shift left, or no effect) of increasing and decreasing the reaction temperature. How does the value of the equilibrium constant depend on temperature?
Problem 7
Problem 21
Write an expression for the equilibrium constant of each chemical equation.
a. SbCl5(g) ⇌ SbCl3(g) + Cl2(g)
b.2 BrNO(g) ⇌ 2 NO(g) + Br2(g)
c. CH4(g) + 2 H2S(g) ⇌ CS2(g) + 4 H2(g)
d. 2 CO(g) + O2(g) ⇌ 2 CO2(g)
Problem 22a
Find and fix each mistake in the equilibrium constant expressions. a. 2 H2S(g) ⇌ 2 H2(g) + S2(g) K = [H2][S2]/[H2S]
Problem 22b
Find and fix each mistake in the equilibrium constant expressions. b. CO(g) + Cl2(g) ⇌ COCl2(g) K = [CO][Cl2]/[COCl2]
Problem 23
When this reaction comes to equilibrium, will the concentrations of the reactants or products be greater? Does the answer to this question depend on the initial concentrations of the reactants and products? A(g)+B(g) ⇌ 2 C(g) Kc = 1.4⨉10-5
Problem 24
Ethene (C2H4) can be halogenated by this reaction: C2H4(g) + X2(g) ⇌ C2H4X2(g) where X2 can be Cl2 (green), Br2 (brown), or I2 (purple). Examine the three figures representing equilibrium concentrations in this reaction at the same temperature for the three different hal- ogens. Rank the equilibrium constants for the three reactions from largest to smallest.
Problem 25a
H2 and I2 are combined in a flask and allowed to react according to the reaction: H2(g) + I2(g) ⇌ 2 HI(g) Examine the figures (sequential in time) and answer the questions: a. Which figure represents the point at which equilibrium is reached?
Problem 26
A chemist trying to synthesize a particular compound attempts two different synthesis reactions. The equilibrium constants for the two reactions are 23.3 and 2.2⨉104 at room temperature. However, upon carrying out both reactions for 15 minutes, the chemist finds that the reaction with the smaller equilibrium constant produces more of the desired product. Explain how this might be possible.
Problem 27a
This reaction has an equilibrium constant of Kp = 2.26⨉104 at 298 K. CO(g) + 2 H2(g) ⇌ CH3OH(g) Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibrium. a. CH3OH(g) ⇌ CO(g) + 2 H2(g)
Problem 27b
This reaction has an equilibrium constant of Kp = 2.26⨉104 at 298 K. CO(g) + 2 H2(g) ⇌ CH3OH(g) Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibrium.
b. 1/2 CO(g) + H2 (g) ⇌ 1/2 CH3OH(g)
Problem 27c
This reaction has an equilibrium constant of Kp = 2.26⨉104 at 298 K. CO(g) + 2 H2(g) ⇌ CH3OH(g) Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibrium.
c. 2 CH3OH(g) ⇌ 2 CO(g) + 4 H2(g)
Problem 28a
This reaction has an equilibrium constant of Kp = 2.2⨉106 at 298 K. 2 COF2(g) ⇌ CO2(g) + CF4(g) Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibrium.
a. COF2 (g) ⇌ 1/2 CO2(g) + 1/2 CF4(g)
Problem 28b
This reaction has an equilibrium constant of Kp = 2.2⨉106 at 298 K. 2 COF2(g) ⇌ CO2(g) + CF4(g) Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibrium.
b. 6 COF2(g) ⇌ 3 CO2(g) + 3 CF4(g)
Problem 28c
This reaction has an equilibrium constant of Kp = 2.2⨉106 at 298 K. 2 COF2(g) ⇌ CO2(g) + CF4(g) Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibrium.
c. 2 CO2(g) + 2 CF4(g) ⇌ 4 COF2(g)
Problem 29
Consider the reactions and their respective equilibrium
constants:
NO(g) + 1/2 Br (g) ⇌ NOBr(g) Kp = 5.3
2 NO(g) ⇌ N2(g) + O2(g) Kp = 2.1⨉1030
Use these reactions and their equilibrium constants to predict
the equilibrium constant for the following reaction: N2(g) + O2(g) + Br2(g) ⇌ 2 NOBr(g)
Problem 31a
Calculate Kc for each reaction. a. I2(g) ⇌ 2I(g) Kp = 6.26⨉10-22 (at 298K)
Problem 32a
Calculate Kp for each reaction. a. N2O4(g) ⇌ 2 NO2(g) Kc = 5.9⨉10-3 (at 298 K)
- Write an equilibrium expression for each chemical equation involving one or more solid or liquid reactants or products: a. CO32-(aq) + H2O(l) ⇌ HCO3-(aq) + OH-(aq) b. 2 KClO3(s) ⇌ 2 KCl(s) + 3 O2(g) c. HF(aq) + H2O(l) ⇌ H3O+(aq) + F-(aq) d. NH3(aq) + H2O(l) ⇌ NH4+(aq) + OH-(aq)
Problem 33
- Find and fix the mistake in the equilibrium expression. PCl5(g) ⇌ PCl3(l) + Cl2(g) Kc = [Cl2]/[PCl5]
Problem 34
- Consider the reaction: CO(g) + 2 H2(g) ⇌ CH3OH(g). An equilibrium mixture of this reaction at a certain temperature has [CO] = 0.105 M, [H2] = 0.114 M, and [CH3OH] = 0.185 M. What is the value of the equilibrium constant (Kc) at this temperature?
Problem 35
- Consider the reaction: NH4HS(s) ⇌ NH3(g) + H2S(g). An equilibrium mixture of this reaction at a certain temperature has [NH3] = 0.278 M and [H2S] = 0.355 M. What is the value of the equilibrium constant (Kc) at this temperature?
Problem 36
Problem 37
Consider the reaction: N2(g) + 3 H2(g) ⇌ 2 NH3(g) Complete the table. Assume that all concentrations are equilibrium concentrations in M.
T (K) [N2] [H2] [NH3] Kc
500 0.115 0.105 0.439 _
575 0.110 _ 0.128 9.6
775 0.120 0.140 _ 0.0584
Problem 38
Consider the following reaction: H2(g) + I2(g) ⇌ 2 HI(g) Complete the table. Assume that all concentrations are equilibrium concentrations in M.
T (°C) [H2] [I2] [HI] Kc
25 0.0355 0.0388 0.922 _
340 _ 0.0455 0.387 9.6
445 0.0485 0.0468 _ 50.2
Problem 39
Consider the reaction: 2 NO(g) + Br2(g) ⇌ 2 NOBr(g) Kp = 28.4 at 298K In a reaction mixture at equilibrium, the partial pressure of NO is 108 torr and that of Br2 is 126 torr. What is the partial pressure of NOBr in this mixture?
Problem 40
Consider the reaction: SO2Cl2(g) ⇌ SO2(g) + Cl2(g) Kp = 2.91⨉103 at 298 K In a reaction at equilibrium, the partial pressure of SO2 is 137 torr and that of Cl2 is 285 torr. What is the partial pressure of SO2Cl2in this mixture?
