Increasing the temperature of a reaction generally increases the reaction rate. Which aspect of collision theory best explains this observation?

Two molecules A and B collide, but no reaction occurs. Which of the following MUST be true?

For an endothermic reaction where, $\Delta H$ represents the enthalpy of the reaction in $kJ/mol,$ the minimum value for the energy of activation will be

A catalyst influences a chemical reaction by affecting which of the following?

If the orientation of colliding molecules is not proper, the collision is termed as:

Consider an endothermic reaction $X o Y$ with the activation energies ${E_b}\;{\rm{and}}\;{E_f}$ for the backward and forward reactions respectively. In general

Consider two reactions, A and B. Reaction A has a higher activation energy than reaction B. Which statement is most likely true?

For a second-order reaction, the slope of the Arrhenius plot $\left( \ln k \ \rm{v/s} \frac{1}{T} \right)$ is determined to be $-10 imes 10^3 \ K$. Calculate the activation energy ($E_a$) for this reaction. (Use $R = 8.314 \ \rm{J} \ {\rm{K}}^{-1} \rm{mol}^{-1}$).

Which of the following theory is not related to chemical kinetics?

A reaction's Arrhenius plot exhibits a slope of $-9 imes 10^3 \ K$. Calculate the activation energy ($E_a$) of this reaction, using $R = 8.314 \ \rm{J} \ {\rm{K}}^{-1} \rm{mol}^{-1}$.

In an Arrhenius plot for a reaction, the slope is found to be $-12 imes 10^3 K$. If the gas constant $R$ is $8.314 \ \rm{J} \ {\rm{K}}^{-1} \rm{mol}^{-1}$, what is the activation energy ($E_a$) of the reaction in $\rm{kJ/mol}$?