State whether the following statements are true or false. If false, explain why. (a) A reaction stops when equilibrium is reached. (b) An equilibrium reaction is not affected by increasing the concentrations of products. (c) If one starts with a higher pressure of reactant, the equilibrium constant will be larger. (d) If one starts with higher concentrations of reactants, the equilibrium concentrations of the products will be larger.

Question

Yandel Mcclain

Chemistry

24 August, 13:26

State whether the following statements are true or false. If false, explain why. (a) A reaction stops when equilibrium is reached. (b) An equilibrium reaction is not affected by increasing the concentrations of products. (c) If one starts with a higher pressure of reactant, the equilibrium constant will be larger. (d) If one starts with higher concentrations of reactants, the equilibrium concentrations of the products will be larger.

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Answers (1)

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Toby · Answer 1

(a) False;

(b) False;

(c) False;

(d) True.

Explanation:

(a) When equilibrium is reached, the forward reaction rate becomes equal to the reverse reaction rate, that's why the molarity of each species remains constant, but reactions don't stop.

(b) According to the principle of Le Chatelier, an increase in molarity of either reactants or products would lead to a disturbance of equilibrium. This disturbance would lead to the shift of equilibrium towards the side which would minimize such a disturbance.

(c) Equilibrium constant is only temperature-dependent, it's independent of molarity, pressure, volume etc. of any species present in the reaction.

(d) The greater the initial molarity of reactants, the more products can be formed, e. g., since the ratio of products to reactants should be kept constant, the larger the amount of reactants, the greater the amount of products formed to keep a constant ratio.