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

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) Please actually draw the diagram, don't just explain how to draw it.

Question

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

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) Please actually draw the diagram, don't just explain how to draw it.

Accepted Answer

∻Solution∻ ‖ 1 ⋮ **Sketch the axes**: Begin by drawing two axes on a graph. The vertical axis represents energy, and the horizontal axis represents the reaction coordinate. ‖ ‖ 2 ⋮ **Label reactants and products**: On the horizontal axis, label the left side as 'Reactants (A + B)' and the right side as 'Products (2C)'. ‖ ‖ 3 ⋮ **Indicate enthalpy change**: Draw a horizontal line on the energy axis for the products that is 25 kJ lower than the reactants, representing the exothermic release of energy, $\Delta H = -25 \mathrm{~kJ}$. ‖ ‖ 4 ⋮ **Draw the transition state**: Plot a peak above the reactants to represent the transition state. The peak's height above the reactants' line is the activation energy for the forward reaction, $E_a = 35.8 \mathrm{~kJ}$. ‖ ‖ 5 ⋮ **Label activation energies**: Label the energy difference between the reactants and the peak as 'Activation Energy (forward) = 35.8 kJ'. For the backward reaction, label the energy difference between the products and the peak as 'Activation Energy (backward)', which is $35.8 \mathrm{~kJ} + 25 \mathrm{~kJ}$. ‖ ‖ 6 ⋮ **Add catalyst effect**: Draw a new peak, lower than the original transition state, to represent the lowered activation energy due to the catalyst. Label this new line 'Catalyst' and the new, lower activation energies for both forward and backward reactions. ‖ ∻Answer∻ ⚹ I cannot physically draw the diagram, but I have provided a detailed description of how to sketch it. ⚹ ∻Key Concept∻ ⚹ An energy diagram visually represents the energy changes during a chemical reaction, including reactants, products, transition states, and activation energies. ⚹ ∻Explanation∻ ⚹ The diagram should show the initial and final energy states of the reactants and products, the energy barrier to be overcome (activation energy), and how a catalyst lowers this barrier.◊How does the addition of a homogeneous catalyst affect the activation energy in a chemical reaction?⍭ Generate me a similar question◊⚹

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