Question

In each of the following three reaction coordinate diagrams, state: (a) Whether the reaction is exothermic or endothermic. (b) Whether the reaction is the slowest, the fastest, or intermediate in rate. (c) If all three reactions have the same entropy change between the reactant and product, which reaction has the largest favorable \(\Delta G^{0}\).

Short answer

Question: Based on the provided reaction diagrams, answer the following questions for each of the three reactions: (a) Determine whether the reaction is exothermic or endothermic. (b) Identify if the reaction is the slowest, the fastest, or intermediate in rate. (c) If all three reactions have the same entropy change between the reactant and product, which reaction has the largest favorable ΔG⁰.

Step-by-step solution

Identify Exothermic and Endothermic Reactions

To determine whether a reaction is endothermic or exothermic, look at the relative energy levels of the reactants and products in the diagram. If the energy level of the product is lower than that of the reactant, the reaction is exothermic. If the energy level of the product is higher than that of the reactant, the reaction is endothermic. ##Step 2: Analyze Reaction Rate##

Analyze Reaction Rate

To determine the reaction rate, observe the height of the energy barriers (activation energy) between the reactants and products in the diagram. Higher energy barriers correspond to slower reaction rates, while lower energy barriers correspond to faster reaction rates. Compare the energy barriers of all three reactions to figure out which is the slowest, the fastest, or intermediate in rate. ##Step 3: Calculate Gibbs Free Energy Change##

Calculate Gibbs Free Energy Change

To find which reaction has the largest favorable \(\Delta G^{0}\), consider the change in enthalpy (\(\Delta H\)) and change in entropy (\(\Delta S\)) for each reaction. The Gibbs free energy change is given by the equation: $$\Delta G^{0} = \Delta H^{0} - T\Delta S^{0}$$ Since all reactions have the same entropy change, the reaction with the most negative value of \(\Delta H^{0}\) (the most exothermic one) will have the largest favorable \(\Delta G^{0}\). ##Step 4: Answer the Questions##

Answer the Questions

Using the analysis from steps 1, 2, and 3, answer the following questions for each of the three reactions: (a) Determine whether the reaction is exothermic or endothermic. (b) Identify if the reaction is the slowest, the fastest, or intermediate in rate. (c) If all three reactions have the same entropy change between the reactant and product, which reaction has the largest favorable \(\Delta G^{0}\).