Consider the equilibrium A 
B in which both the forward and reverse reactions are elementary (single-step) reactions. Assume that the only effect of a catalyst on the reaction is to lower the activation energies of the forward and reverse reactions, as shown in Figure 15.14. Using the Arrhenius equation (Section 14.5), prove that the equilibrium constant is the same for the catalyzed reaction as for the uncatalyzed one.
Consider the equilibrium A B in which both the forward and reverse reactions are elementary (single-step) reactions. Assume that the only effect of a catalyst on the reaction is to lower the activation energies of the forward and reverse reactions, as shown in Figure 15.14. Using the Arrhenius equation (Section 14.5), prove that the equilibrium constant is the same for the catalyzed reaction as for the uncatalyzed one.
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Related questions
The use of a catalyst causes the rate constant for the reaction R→P to increase by a factor of exactly 250 at 298 K. Which one of the following statements best describes the effect of the catalyst?
Assume that the rate constant for the reaction obeys the Arrhenius equation and that the Arrhenius pre-exponential factors are the same for both the catalyzed and uncatalyzed reactions.
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The catalyst increases the activation energy by 13.7 kJ mol-1 |
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The catalyst increases the activation energy by 6.43 kJ mol-1 |
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The catalyst decreases the activation energy by 13.7 kJ mol-1 |
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The catalyst decreases the activation energy by 6.43 kJ mol-1 |
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The catalyst decreases the enthalpy change by 11.8 kJ mol-1 |
