For the single step reaction:
$$
A+B \rightarrow 2 C+25 \mathrm{~kJ}
$$

If the activation energy for this reaction is $35.8 \mathrm{~kJ}$, sketch an energy vs. reaction co-ordinate diagram for this reaction. Be sure to label the following on your diagram: each of the axes, reactant compounds and product compounds, enthalpy of reaction, activation energy of the forward reaction with the correct value, activation energy of the backwards reaction with the correct value and the transition state. (8 marks)

On the same sketch you drew, after the addition of a homogeneous catalyst, show how it would change the graph. Label any new line "catalyst" and label any new activation energy. (2 marks)

Question

For the single step reaction:
$$
A+B \rightarrow 2 C+25 \mathrm{~kJ}
$$

If the activation energy for this reaction is $35.8 \mathrm{~kJ}$, sketch an energy vs. reaction co-ordinate diagram for this reaction. Be sure to label the following on your diagram: each of the axes, reactant compounds and product compounds, enthalpy of reaction, activation energy of the forward reaction with the correct value, activation energy of the backwards reaction with the correct value and the transition state. (8 marks)

On the same sketch you drew, after the addition of a homogeneous catalyst, show how it would change the graph. Label any new line "catalyst" and label any new activation energy. (2 marks)

Accepted Answer

∻Solution∻ ‖ 1 ⋮ **Sketch the energy vs. reaction coordinate diagram**: Begin by drawing a horizontal axis to represent the reaction coordinate and a vertical axis to represent the energy. ‖ ‖ 2 ⋮ **Label the axes**: Label the horizontal axis as 'Reaction Coordinate' and the vertical axis as 'Energy'. ‖ ‖ 3 ⋮ **Plot the reactants and products**: Mark the energy level of the reactants, $A$ and $B$, on the left side of the diagram and the energy level of the products, $2C$, on the right side. The products are lower in energy by $25 \mathrm{~kJ}$ compared to the reactants, indicating an exothermic reaction. ‖ ‖ 4 ⋮ **Indicate the enthalpy of reaction**: Draw a horizontal arrow pointing downwards from the energy level of the reactants to the energy level of the products and label it as $\Delta H = -25 \mathrm{~kJ}$. ‖ ‖ 5 ⋮ **Mark the transition state**: At a point higher than the reactants' energy, draw a peak to represent the transition state. ‖ ‖ 6 ⋮ **Label the activation energy for the forward reaction**: Draw an arrow from the reactants' energy level to the peak of the transition state and label it as $E_a (forward) = 35.8 \mathrm{~kJ}$. ‖ ‖ 7 ⋮ **Label the activation energy for the backward reaction**: Draw an arrow from the products' energy level to the peak of the transition state and label it as $E_a (backward) = 35.8 \mathrm{~kJ} + 25 \mathrm{~kJ}$. ‖ ‖ 8 ⋮ **Add a catalyst to the diagram**: Draw a new curve from the reactants to the products that passes through a lower point than the original transition state to represent the lowered activation energy due to the catalyst. Label this new line as "catalyst". ‖ ‖ 9 ⋮ **Label the new activation energies**: Label the new, lower activation energies for both the forward and backward reactions with the catalyst in place. ‖ ∻Answer∻ ⚹ A correctly labeled energy vs. reaction coordinate diagram with a lower activation energy path due to the catalyst. ⚹ ∻Key Concept∻ ⚹ Energy diagrams illustrate the energy changes during a chemical reaction and the effect of a catalyst on lowering activation energy. ⚹ ∻Explanation∻ ⚹ The diagram shows the energy of reactants and products, the enthalpy change of the reaction, the activation energies for both forward and backward reactions, and how a catalyst provides an alternative pathway with a lower activation energy. ⚹◊How does the addition of a homogeneous catalyst affect the activation energy of a single step reaction?⍭ Generate me a similar question◊

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