If the activation energy for a given compound is found to be 103 kJ/mol,with a frequency factor of 4.0 × 10¹³ s^-1,what is the rate constant for this reaction at 398 K?

Question

Quizplus · Accepted Answer

The rate constant (k) can be calculated using the Arrhenius equation: $k = A \exp\left(-\frac{E_a}{RT}\right)$, where $A$ is the frequency factor, $E_a$ is the activation energy in J/mol (103 kJ/mol = 103,000 J/mol), $R$ is the gas constant (8.314 J/mol·K), and $T$ is the temperature in Kelvin (398 K). Plugging in the values: $k = 4.0 \times 10^{13} \exp\left(-\frac{103,000}{8.314 \times 398}\right)$, which calculates to approximately 1.2 s^-1, making option A correct.

If the Activation Energy for a Given Compound Is Found