Which statements are true about reversible reactions?

Select all the correct answers,

Reversible reactions can reach equilibrium only when a catalyst is used.

Reversible reactions exhibit a faster rate of forward reaction than reverse reaction at equilibrium.

Reversible reactions are more product favored than reactant favored,

Reversible reactions exhibit the same reaction rate for forward and reverse reactions at equilibrium,

Reversible reactions exhibit constant concentrations of reactants and products at equilibrium

Question

Cody Carroll

Chemistry

28 February, 12:41

Which statements are true about reversible reactions?

Select all the correct answers,

Reversible reactions can reach equilibrium only when a catalyst is used.

Reversible reactions exhibit a faster rate of forward reaction than reverse reaction at equilibrium.

Reversible reactions are more product favored than reactant favored,

Reversible reactions exhibit the same reaction rate for forward and reverse reactions at equilibrium,

Reversible reactions exhibit constant concentrations of reactants and products at equilibrium

+3

Answers (2)

Know the Answer?

Amani Byrd · Answer 1

Reversible reactions exhibit the same reaction rate for forward and reverse reactions at equilibrium.

Reversible reactions exhibit constant concentrations of reactants and products at equilibrium

Explanation:

A reversible reaction is a reaction that can proceed in both forward and backward direction.

Equilibrium is attained in a chemical system when there is no observable change in the properties of the system.

At equilibrium, a reversible reaction is occurring in at same rate. That is, the forward and backward reaction is occurring at the same rate. As the rate of the forward and backward reaction remains the same, the concentrations of the reactants and products will also be the same in order for the equilibrium to be maintained.

Jimmy Collier · Answer 2

Option D is correct. Reversible reactions exhibit the same reaction rate for forward and reverse reactions at equilibrium.

Explanation:

Reversible reactions can be illustrated with the equation below:

A + B ⇄ C + D

The reactants, A and B reacts to give the products, C and D. The products then react to give back the reactants.

Reversible reactions can reach equilibrium without a catalyst. Catalyst only speed up the rate at which the equilibrium is reached. This makes option A wrong.

In reversible reaction, both the forward and backward rate are equal. This makes option B wrong.

Option C is also wrong because no side (reactant of product) is favoured in a reversible reaction, unless the system is disturbed.

Option D is correct. Reversible reactions exhibit the same reaction rate for forward and reverse reactions at equilibrium.

option E is wrong.