Which statement best describes the relationship between activation energy and reaction rate?

For the reaction $A o B$, the enthalpy of reaction is $-4.2 ext{ kJ mol}^{-1}$ and the enthalpy of activation is $9.6 ext{ kJ mol}^{-1}$. Which potential energy profile correctly represents this reaction?

The ${E_a}$ of exothermic reaction, $A o B$ is $80\,\,KJ/mol$. Heat of reaction is $20\,\,KJ/mol$. ${E_a}$ for the reaction $B o A$ will be

Collision theory explains reaction rates in terms of:

The rate of reaction increases with temperature due to

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

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 $\rm{kJ/mol}$?

According to collision theory, for a reaction to occur, colliding molecules must have:

If $X$ is the total number of collisions which a gas molecule register with others per unit time under particular conditions, then the collision frequency of the gas containing $N$ molecules per unit volume is

An endothermic reaction ${A o B}$ has an activation energy of $15{\rm{ }}\;kcal/mol$ and the energy of reaction is $5\;{\rm{ }}kcal/mol$. The activation energy for the reaction $B o A$ is

The threshold energy of a chemical reaction depends upon: