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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 31b
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 32a
Calculate Kp for each reaction. a. N2O4(g) ⇌ 2 NO2(g) Kc = 5.9⨉10-3 (at 298 K)
Problem 32b
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)
- 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
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?
- Consider the reaction: Fe3+ (aq) + SCN- (aq) ⇌ FeSCN2+ (aq). A solution is made containing an initial [Fe3+] of 1.0*10^-3 M and an initial [SCN-] of 8.0*10^-4 M. At equilibrium, [FeSCN2+] = 1.7*10^-4 M. Calculate the value of the equilibrium constant (Kc).
Problem 43
- Consider the reaction: SO2Cl2(g) ⇌ SO2(g) + Cl2(g). A reaction mixture is made containing an initial [SO2Cl2] of 0.020 M. At equilibrium, [Cl2] = 1.2*10^-2 M. Calculate the value of the equilibrium constant (Kc).
Problem 44
- Consider the reaction: H2(g) + I2(g) ⇌ 2 HI(g). A reaction mixture in a 3.67-L flask at a certain temperature initially contains 0.763 g H2 and 96.9 g I2. At equilibrium, the flask contains 90.4 g HI. Calculate the equilibrium constant (Kc) for the reaction at this temperature.
Problem 45
- Consider the reaction: CO(g) + 2 H2(g) ⇌ CH3OH(g). A reaction mixture in a 5.19-L flask at a certain temperature contains 26.9 g CO and 2.34 g H2. At equilibrium, the flask contains 8.65 g CH3OH. Calculate the equilibrium constant (Kc) for the reaction at this temperature.
Problem 46
Problem 47
Consider the reaction: NH4HS(s) ⇌ NH3(g) + H2S(g) At a certain temperature, Kc = 8.5⨉10-3. A reaction mixture at this temperature containing solid NH4HS has [NH3] = 0.166 M and [H2S] = 0.166 M. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached?
Problem 49
Silver sulfate dissolves in water according to the reaction: Ag2SO4(s) ⇌ 2 Ag+(aq) + SO42-(aq) Kc = 1.1⨉10-5 at 298 K. A 1.5-L solution contains 6.55 g of dissolved silver sulfate. If additional solid silver sulfate is added to the solution, will it dissolve?
Problem 51
Consider the reaction and the associated equilibrium constant: aA(g) ⇌ bB(g) Kc = 4.0 Find the equilibrium concentrations of A and B for each value of a and b. Assume that the initial concentration of A in each case is 1.0 M and that no B is present at the beginning of the reaction. c. a=1;b=2
- Consider the reaction and the associated equilibrium constant: aA(g) + bB(g) ⇌ cC(g) with Kc = 5.0. Find the equilibrium concentrations of A, B, and C for the given values of a, b, and c. Assume that the initial concentrations of A and B are each 1.0 M and that no product is present at the beginning of the reaction. Calculate the equations for x without solving them for the following cases: a) a=1, b=1, c=2; b) a=1, b=1, c=1; c) a=2, b=1, c=1.
Problem 52
Problem 53
For the reaction shown here, Kc = 0.513 at 500 K. N2O4(g) ⇌ 2 NO2(g) If a reaction vessel initially contains an N2O4 concentration of 0.0500 M at 500 K, what are the equilibrium concentrations of N2O4 and NO2 at 500 K?
Problem 54
For the reaction shown here, Kc = 255 at 1000 K. CO(g) + Cl2(g) ⇌ COCl2(g) If a reaction mixture initially contains a CO concentration of 0.1500 M and a Cl2 concentration of 0.175 M at 1000 K, what are the equilibrium concentrations of CO, Cl2, and COCl2 at 1000 K?
- Consider the reaction: NiO(s) + CO(g) ⇌ Ni(s) + CO2(g) Kc = 4.0 * 10^3 at 1500 K. If a mixture of solid nickel(II) oxide and 0.20 M carbon monoxide comes to equilibrium at 1500 K, what is the equilibrium concentration of CO2?
Problem 55
- Consider the reaction: CO(g) + H2O(g) ⇌ CO2(g) + H2(g) Kc = 102 at 500 K. If a reaction mixture initially contains 0.110 M CO and 0.110 M H2O, what will the equilibrium concentration of each of the reactants and products be?
Problem 56
Problem 57
Consider the reaction: HC2H3O2(aq) + H2O(l) ⇌ H3O+(aq) + C2H3O2-(aq) Kc = 1.8⨉10-5 at 25°C If a solution initially contains 0.210 M HC2H3O2, what is the equilibrium concentration of H3O+ at 25 °C?
Problem 58
Consider the reaction: SO2Cl2(g) ⇌ SO2(g) + Cl2(g) Kc = 2.99⨉10-7 at 227 °C If a reaction mixture initially contains 0.175 M SO2Cl2, what is the equilibrium concentration of Cl2 at 227 °C?