Question

The slope of Arrhenius Plot (\(\ln k\) v/s \(\frac{1}{T}\)) of the first-order reaction is \(-5 \times 10^3 \, K\). The value of \(E_a\) of the reaction is. Choose the correct option for your answer. [Given \(R = 8.314 \, JK^{-1}mol^{-1}\)]

• A. \(166 \, kJ \, mol^{-1}\)
• B. \(-83 \, kJ \, mol^{-1}\)
• C. \(41.5 \, kJ \, mol^{-1}\)
• D. \(83.0 \, kJ \, mol^{-1}\)

Hint:

For Arrhenius plots: \[ \ln k \text{ vs } \frac{1}{T} \Rightarrow \text{Slope} = -\frac{E_a}{R} \] while \[ \log k \text{ vs } \frac{1}{T} \Rightarrow \text{Slope} = -\frac{E_a}{2.303R} \] Always check whether the logarithm is natural log or common log.

Answer 1

The Correct Option is C