Seema Saini Solutions for Chapter: Chemical Kinetics, Exercise 5: DPP 4.5

For a zero-order reaction, will the molecularity be equal to zero? Explain.

A ${\mathrm{I}}^{\mathrm{st}}$ order reaction is $50\%$ complete in $30$ minutes at $27°\mathrm{C}$ and in $10$ minutes at $47°\mathrm{C}$. Calculate the energy of activation for the reaction.

A${\mathrm{I}}^{\mathrm{st}}$ order reaction is $50\%$ complete in $30$ minutes at $27°\mathrm{C}$ and in $10$ minutes at $47°\mathrm{C}$. Calculate the energy of activation for the reverse reaction if heat of reaction is $-500 \mathrm{kJ} {\mathrm{mol}}^{-1}$.

Arrhenius equation may be written as

Rate constant for a reaction varies with temperature as $\mathrm{lnk} \left({\sec }^{-1}\right)=14.34-\frac{1.25\times {10}^4}{\mathrm{T}}$. Which among the following statement(s) is/are correct?

For a reaction, activation energy for the forward reaction is $50 \mathrm{kJ}$ and for the backward reaction is $30 \mathrm{kJ}$. Which of the following are true for the reaction?

During decomposition of an activated complex

Which of the following statements is/are correct?