Problem 4 In general, how does the rate of... [FREE SOLUTION]

Chapter 39: Problem 4

In general, how does the rate of the forward reaction \((\mathrm{Y} \rightarrow \mathrm{Z})\) at equilibrium compare to the rate of the reverse reaction \((\mathrm{Z} \rightarrow \mathrm{Y})\) at equilibrium?

Short Answer

Expert verified

At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction.

Step by step solution

Understanding Equilibrium

In a chemical reaction, equilibrium refers to the state at which both the reactants and products are present in concentrations that have no further tendency to change with time. This happens when the rate of the reaction producing the reactants (the reverse reaction, \(Z \rightarrow Y\)) is equal to the rate of the reaction producing the products (the forward reaction, \(Y \rightarrow Z\)).

Analyzing the Rates of Reaction

At the point of equilibrium, the rate at which the reactants \(Y\) are converted into the products \(Z\) (that is, the \(Y \rightarrow Z\) reaction) equals the rate at which the products \(Z\) are converted back into the reactants \(Y\) (the \(Z \rightarrow Y\) reaction). These two rates equate because, in equilibrium, the proportions of the reactants and products do not change over time.

Comparing the Forward and Reverse Reactions at Equilibrium

Therefore, at equilibrium, the rate of the forward reaction (\(Y \rightarrow Z\)) equals the rate of the reverse reaction (\(Z \rightarrow Y\)). There is no net change in the concentrations of the reactants and products, although both the forward and reverse reactions continue to occur.

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In general, how does the rate of the forward reaction \((\mathrm{Y} \rightarrow \mathrm{Z})\) at equilibrium compare to the rate of the reverse reaction \((\mathrm{Z} \rightarrow \mathrm{Y})\) at equilibrium?

Short Answer

Step by step solution

Understanding Equilibrium

Analyzing the Rates of Reaction

Comparing the Forward and Reverse Reactions at Equilibrium

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