The rate constant of a certain reaction is 4.7×10^{- 3} s^{- 1} at 18.0 ° C and the energy of activation is 33.6 kJ/mol. What is the value of a second rate constant for this same reaction at 65.0 ° C?

Question

Quizplus · Accepted Answer

The Arrhenius equation, $k = A e^{-E_a/(RT)}$, can be used to calculate the rate constant at a different temperature, where $E_a$ is the activation energy, $R$ is the gas constant (8.314 J/mol·K), and $T$ is the temperature in Kelvin. Given the activation energy and the initial rate constant, we can use the ratio of rate constants at two temperatures to find the second rate constant without needing the pre-exponential factor $A$. The correct answer must be calculated based on the change in temperature from 18.0 °C (291.15 K) to 65.0 °C (338.15 K), using the given activation energy. The calculation involves using the Arrhenius equation to relate the two temperatures and the given activation energy, leading to the selection of the correct rate constant value.

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