Which of the following statements is/are wrong?

Question

Which of the following statements is/are wrong? (A) At equilibrium concentrations of reactants and products become constant because the reaction stops (B) Addition of catalyst speeds up the forward reaction more than the backward reaction (C) Equilibrium constant of an exothermic reaction decreases with increase of temperature (D) Kp is always greater than Kc

Tardigrade Admin · Accepted Answer

Correct answer is (a) At equilibrium concentrations of reactants and products become constant because the reaction stopsCorrect answer is (b) Addition of catalyst speeds up the forward reaction more than the backward reactionCorrect answer is (d) Kp is always greater than Kc

Q. Which of the following statements is/are wrong?

At equilibrium concentrations of reactants and products become constant because the reaction stops

Addition of catalyst speeds up the forward reaction more than the backward reaction

Equilibrium constant of an exothermic reaction decreases with increase of temperature

$K_{p}$ is always greater than $K_{c}$

Correct answer is (a) At equilibrium concentrations of reactants and products become constant because the reaction stopsCorrect answer is (b) Addition of catalyst speeds up the forward reaction more than the backward reactionCorrect answer is (d) $K_{p}$ is always greater than $K_{c}$