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In a reversible reaction at equilibrium, which of the following statements is tr

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Question: In a reversible reaction at equilibrium, which of the following statements is true?

Options:

  1. The rate of the forward reaction is equal to the rate of the reverse reaction.
  2. The concentration of reactants is greater than products.
  3. The reaction has stopped completely.
  4. The temperature remains constant.

Correct Answer: The rate of the forward reaction is equal to the rate of the reverse reaction.

Solution: 

At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction, which means the concentrations of reactants and products remain constant over time.

In a reversible reaction at equilibrium, which of the following statements is tr

Practice Questions

Q1
In a reversible reaction at equilibrium, which of the following statements is true?
  1. The rate of the forward reaction is equal to the rate of the reverse reaction.
  2. The concentration of reactants is greater than products.
  3. The reaction has stopped completely.
  4. The temperature remains constant.

Questions & Step-by-Step Solutions

In a reversible reaction at equilibrium, which of the following statements is true?
  • Step 1: Understand that a reversible reaction can go in both directions: from reactants to products and from products to reactants.
  • Step 2: Know that equilibrium is a state where the forward and reverse reactions are happening at the same rate.
  • Step 3: Realize that when the rates are equal, the concentrations of reactants and products do not change over time.
  • Step 4: Conclude that at equilibrium, the statement 'the rate of the forward reaction equals the rate of the reverse reaction' is true.
  • Equilibrium in Reversible Reactions – At equilibrium, the rates of the forward and reverse reactions are equal, leading to constant concentrations of reactants and products.
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