In a reversible reaction at equilibrium, which of the following statements is true?
Practice Questions
1 question
Q1
In a reversible reaction at equilibrium, which of the following statements is true?
The rate of the forward reaction is equal to the rate of the reverse reaction.
The concentration of reactants is greater than products.
The reaction has stopped completely.
The temperature remains constant.
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.
Questions & Step-by-step Solutions
1 item
Q
Q: In a reversible reaction at equilibrium, which of the following statements is true?
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.
Steps: 4
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.
