In general, as activation energy increases, reaction rate ___. a) goes down if t
ID: 500086 • Letter: I
Question
In general, as activation energy increases, reaction rate ___. a) goes down if the reaction is exothermic B) goes down if the reaction is endothermic C) stays-the-same regardless of whether the reaction is exothermic or endothermic D) goes down regardless of whether the reaction is exothermic or endothermic E) none of the above Which of the following expressions is the correct equilibrium-constant expression for the equilibrium between nitrogen and nitrogen dioxide? N_2O_4(g) 2NO_2(g) A) [NO_2][N_2O_4] B) [NO_2]^2/[N_2O_4] C) [NO_2]/[N_2O_4]^2 D) [NO_2][N_2O_54] E) [NO_2]^2/[N_2O_4] The K_eq for the equilibrium below is 7.52 times 10^-2 at 480.0 degree C. 2CI_2(g) + 2H_2O(g) 4HCI(g) + O_2(g) What is the value of K_eq at this temperature for the following reaction? 4HCI(g) + O_2(g) 2CI_2(g) + 2H_2O(g) Solving procedures:Explanation / Answer
1) the activation energy is the amount of energy required by reactants to undergo reaction
so lower the activation energy higher the rate of reaction
so if activation energy is increases the reaction rate goes down irrespective of the exothermic or endothermic reaction
2) Keq = Product of concentration of products / Product of concentration of reactants
Keq = [NO2]^2 / [N2O4]
3) the other reaction is just reverse of previous reaction given
So here
K(1) = 1/K(2)
K(2) = 1/ K(1) = 1 / 7.52 X 10^-2 = 13.297