The minimum energy necessary to permit a reaction is

For the reaction $A \to B$,$K_1 = 10^8 \, e^{-6000/8.34T}$ and for the reaction $P \to Q$,$K_2 = 10^{10} \, e^{-8000/8.34T}$. At what temperature $T$ will $K_1 = K_2$ (in $K$)?

The activation energy for the reaction $X \rightarrow Y$ is $150 \text{ kJ mol}^{-1}$. The change in enthalpy for the above reaction is $-135 \text{ kJ mol}^{-1}$. What is the activation energy for the reverse reaction $Y \rightarrow X$?

For an exothermic reaction,the following two steps are involved:
Step $1$: $A + B \to I$ $(slow)$
Step $2$: $I \to AB$ $(fast)$
Which of the following graphs correctly represents this reaction?

In collision theory of chemical reaction,$Z_{AB}$ represents

For an endothermic reaction,$\Delta H$ represents the enthalpy of the reaction in $kJ \ mol^{-1}$. The minimum amount of activation energy will be