Textbook Question
Consider this energy diagram:
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b. Label the reactants, products, and intermediates.
15. Chemical Kinetics
Energy Diagrams
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The activation energy of a reaction is 3.5 kJ/mol and the change in enthalpy for the forward reaction is -67.2 kJ/mol. What is the activation energy of the reverse reaction?
A
63.7 kJ/mol
B
70.7 kJ/mol
C
67.2 kJ/mol
D
3.5 kJ/mol
Verified step by step guidance1
Understand that the activation energy (Ea) is the minimum energy required for a reaction to occur. For a reverse reaction, the activation energy is different from the forward reaction.
Recall that the activation energy of the reverse reaction can be calculated using the relationship: Ea(reverse) = Ea(forward) + ΔH, where ΔH is the change in enthalpy for the forward reaction.
Identify the given values: Ea(forward) = 3.5 kJ/mol and ΔH = -67.2 kJ/mol. Note that ΔH is negative because the forward reaction is exothermic.
Substitute the given values into the equation: Ea(reverse) = 3.5 kJ/mol + (-67.2 kJ/mol).
Calculate the result to find the activation energy of the reverse reaction. Remember to consider the sign of ΔH when performing the calculation.
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