1. Which of the following does a K = 4.3x10-3 signify? a. The reactants are of significantly lower amounts than the products. b. The reverse rate is higher than the forward rate. c. The formation of reactants is favored when the rates are equal. d. The rate of reaction is small. 2. For the reaction: 2A(g) + B(g) ↔ 2 C(g) Kc = 25 If the system contains [A] = 0.15 M, [B] = 0.35 M, and [C] = 0.75 M, which of the following is TRUE? a. The forward rate of reaction will be higher than the reverse rate. b. The forward rate of reaction will be lower than the reverse rate. c. The rates of the forward and reverse reactions will be equal. 3. Given the reaction: 2A(g) + B(g) ↔ 2 C(g) Kc = 25 a. What is the value of the equilibrium constant for the reaction: A(g) + ½ B(g) ↔ C(g) Kc = ?? b. What is the value of the equilibrium constant for the reaction: 2 C(g) ↔ 2 A(g) + B(g) Kc = ??
1. Which of the following does a K = 4.3x10-3 signify? a. The reactants are of significantly lower amounts than the products. b. The reverse rate is higher than the forward rate. c. The formation of reactants is favored when the rates are equal. d. The rate of reaction is small. 2. For the reaction: 2A(g) + B(g) ↔ 2 C(g) Kc = 25 If the system contains [A] = 0.15 M, [B] = 0.35 M, and [C] = 0.75 M, which of the following is TRUE? a. The forward rate of reaction will be higher than the reverse rate. b. The forward rate of reaction will be lower than the reverse rate. c. The rates of the forward and reverse reactions will be equal. 3. Given the reaction: 2A(g) + B(g) ↔ 2 C(g) Kc = 25 a. What is the value of the equilibrium constant for the reaction: A(g) + ½ B(g) ↔ C(g) Kc = ?? b. What is the value of the equilibrium constant for the reaction: 2 C(g) ↔ 2 A(g) + B(g) Kc = ??
1. Which of the following does a K = 4.3x10-3 signify? a. The reactants are of significantly lower amounts than the products. b. The reverse rate is higher than the forward rate. c. The formation of reactants is favored when the rates are equal. d. The rate of reaction is small. 2. For the reaction: 2A(g) + B(g) ↔ 2 C(g) Kc = 25 If the system contains [A] = 0.15 M, [B] = 0.35 M, and [C] = 0.75 M, which of the following is TRUE? a. The forward rate of reaction will be higher than the reverse rate. b. The forward rate of reaction will be lower than the reverse rate. c. The rates of the forward and reverse reactions will be equal. 3. Given the reaction: 2A(g) + B(g) ↔ 2 C(g) Kc = 25 a. What is the value of the equilibrium constant for the reaction: A(g) + ½ B(g) ↔ C(g) Kc = ?? b. What is the value of the equilibrium constant for the reaction: 2 C(g) ↔ 2 A(g) + B(g) Kc = ??
1. Which of the following does a K = 4.3x10-3 signify? a. The reactants are of significantly lower amounts than the products. b. The reverse rate is higher than the forward rate. c. The formation of reactants is favored when the rates are equal. d. The rate of reaction is small. 2. For the reaction: 2A(g) + B(g) ↔ 2 C(g) Kc = 25 If the system contains [A] = 0.15 M, [B] = 0.35 M, and [C] = 0.75 M, which of the following is TRUE? a. The forward rate of reaction will be higher than the reverse rate. b. The forward rate of reaction will be lower than the reverse rate. c. The rates of the forward and reverse reactions will be equal. 3. Given the reaction: 2A(g) + B(g) ↔ 2 C(g) Kc = 25 a. What is the value of the equilibrium constant for the reaction: A(g) + ½ B(g) ↔ C(g) Kc = ?? b. What is the value of the equilibrium constant for the reaction: 2 C(g) ↔ 2 A(g) + B(g) Kc = ?? 4. Given the reaction: 3X(g) + Y(g) ↔ 2 Z(g) + W(g) Which of the following is true? a. Kc > Kp b. Kc < Kp c. Kc = Kp 5. For the reaction: 2 X(s) + 3 Y(g) ↔ 2 Z(s) Kc = ??? At equilibrium, the system contains [Y] = 0.0025 M. The amounts of [X(s)] = 100 mol/L and [Z(s)] = 395 mol/L. What is the value of the equilibrium constant? 6. For the reaction: 3A(g) + 2B(g) ↔ 3 C(g) Kc = 0.0245 At equilibrium, the system contains [A] = 0.075 M and [B] = 0.115 M. What is the concentration of C at equilibrium (in M)? 7. Given the reaction A(g) + 3B(g) ↔ 2 C(g) Kc = ??? Initially, only 0.200 M of C(g) is present. At equilibrium, 0.050 M of A is present. What is the value of the equilibrium constant?
Definition Definition Study of the speed of chemical reactions and other factors that affect the rate of reaction. It also extends toward the mechanism involved in the reaction.
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