TS EAMCET · Chemistry · Chemical Kinetics
For a first order reaction, a plot of \(\ln k\left(y\right.\)-axis) and \(\frac{1}{T}\) ( \(x\)-axis) gave the straight line with slope equal to \(-10^3 k\) and intercept equal to 2.303 (on \(y\)-axis). What is the activation energy ( \(E_a\) in \(\mathrm{kJ} \mathrm{mol}^{-1}\) ) of the reaction? (Given \(R=8.314\) \(\mathrm{J} \mathrm{mol}^{-1} \mathrm{~K}^{-1}\) )
- A 8.314
- B 2303
- C 2.303
- D 83.14
Answer & Solution
Correct Answer
(A) 8.314
Step-by-step Solution
Detailed explanation
According to Arrhenius Theory, \(\ln \mathrm{k}=\ln \mathrm{A}-\frac{\mathrm{E}_{\mathbf{a}}}{\mathbf{R t}}\) straight line graph \(\begin{aligned} & y=m x+c \\ & \text { slope }(m)=-\frac{E_a}{R} \\ & \text { Intercept }(c)=\ln A \end{aligned}\)…
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