ExamBro
ExamBro
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 \(R=8.314\) \(\mathrm{J} \mathrm{mol}^{-1} \mathrm{~K}^{-1}\) )

  1. A 8.314
  2. B 2303
  3. C 2.303
  4. D 83.14
Verified Solution

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 \(\begin{aligned} & y=m x+c \\ & \text { slope }(m)=-\frac{E_a}{R} \\ & \text { Intercept }(c)=\ln A \end{aligned}\)…
Same subject
Explore more questions on app