Activation Energy From Rate Constants

Question

The table shows the rate constant, k, for a reaction at different temperatures. Using the data and the Arrhenius equation, $$\ln{(k_2/k_1)} = -\frac{E_a}{R}(1/T_2 - 1/T_1)$$, estimate the activation energy, $E_a$, in J/mol. Use R = 8.314 J/(mol·K).

| Temperature (K) | k (s^-1) |
|-----------------|----------|
| 290             | 0.0020   |
| 300             | 0.0050   |
| 310             | 0.0120   |

Accepted Answer

Approximately $$6.7 	imes 10^4\,J/mol$$.

Answer

Approximately $$1.2 	imes 10^5\,J/mol$$.

Answer

Approximately $$6.7 	imes 10^3\,J/mol$$, which likely results from a misapplication of the temperature conversion in the Arrhenius equation.

Answer

Approximately $$1.2 	imes 10^4\,J/mol$$.

Activation Energy From Rate Constants

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