The following graph shows two different reaction pathways for the same overall reaction at the same temperature. Is each of the following statements true or false? (b) For both paths, the rate of the reverse reaction is slower than the rate of the forward reaction.

Verified step by step guidance

1. Step 1: Identify the forward and reverse reactions on the graph. The forward reaction progresses from left to right, while the reverse reaction progresses from right to left.
2. Step 2: Observe the energy barriers (activation energies) for both the forward and reverse reactions. The activation energy is the peak of the curve minus the energy of the reactants for the forward reaction, and the peak of the curve minus the energy of the products for the reverse reaction.
3. Step 3: Compare the activation energies for the forward and reverse reactions for both pathways. The pathway with the lower activation energy will have a faster reaction rate.
4. Step 4: Determine if the activation energy for the reverse reaction is higher than that for the forward reaction in both pathways. If it is, then the rate of the reverse reaction is slower than the rate of the forward reaction.
5. Step 5: Conclude whether the statement 'For both paths, the rate of the reverse reaction is slower than the rate of the forward reaction' is true or false based on the comparison of activation energies.

Key Concepts

Reaction Pathways

Reaction pathways illustrate the energy changes that occur during a chemical reaction. They depict the energy of reactants, products, and the transition states, which are the highest energy points along the pathway. Understanding these pathways helps in analyzing how different conditions or catalysts can affect the rate and mechanism of a reaction.

Forward and Reverse Reactions

In a chemical reaction, the forward reaction refers to the process where reactants are converted into products, while the reverse reaction is the conversion of products back into reactants. The rates of these reactions can differ based on the energy barriers depicted in the reaction pathway, influencing the overall dynamics of the reaction system.

Activation Energy

Activation energy is the minimum energy required for a reaction to occur. It is represented by the height of the energy barrier between reactants and the transition state in a reaction pathway. A higher activation energy typically results in a slower reaction rate, which is crucial for determining whether the forward or reverse reaction is favored under specific conditions.