The rate of the forward reaction is equal to the rate of the reverse reaction
Explanation:
Equilibrium is a condition in which the net force for change is zero.
In chemistry, equilibrium exists when reactant concentrations in a reaction are not changing. This condition means the reaction proceeding left to right in the reaction equation is producing products at the same rate those products are being used up by the reaction proceeding right to left. In short, the rate of the forward reaction is equal to the rate of the reverse reaction.
Answer: The rate of the forward reaction is equal to the rate of the reverse reaction.
Explanation: In a reversible chemical reaction, chemical equilibrium is a point at which there will be no further change in the concentrations of both the reactants and products.
Consider this reaction: A+B <=> C+D
At the starting of the reaction, the rate of the forward reaction will be rapid because the concentrations of A and B are at their peak, at this point the rate of the reverse reaction is slow because virtually no molecules of C and D have been formed. As the reaction proceeds, the rate of the forward reaction decreases as A and B are used up and the rate of the reverse reaction increases as more C and D are formed. A point will reach when the rates of both reactions will be the same and there will be no further change in the concentrations of the reactants and products unless the conditions of the reaction are changed. This point is described as equilibrium.
I don't think so. "It's not a matter of pigment discrimination: Red and yellow bell peppers are essentially just green peppers that have been allowed to ripen"
