The minimum energy that reactant molecules must possess at the time of collision for an effective collision is called ...

In the reaction of decomposition of reactant $A$ into product,the rate constant is $4.5 \times 10^{-3} \ s^{-1}$ at $283 \ K$ temperature and energy of activation is $60 \ kJ \ mol^{-1}$. At which temperature will the value of rate constant $K$ be $3 \times 10^{10} \ s^{-1}$ (in $K$)?

The temperature dependence of the rate constant $(k)$ of a chemical reaction is expressed by the Arrhenius equation,$k = A \cdot e^{-E^*/RT}$. The activation energy $(E^*)$ of the reaction can be calculated by plotting:

The energies of activation for forward and reverse reactions for $A_2 + B_2 \rightleftharpoons 2AB$ are $180 \, kJ \, mol^{-1}$ and $200 \, kJ \, mol^{-1}$ respectively. The presence of a catalyst lowers the activation energy of both (forward and reverse) reactions by $100 \, kJ \, mol^{-1}.$ The enthalpy change of the reaction $(A_2 + B_2 \rightarrow 2AB)$ in the presence of a catalyst will be (in $kJ \, mol^{-1}$)

What is the role of a catalyst in a chemical reaction?

In the Arrhenius equation,the fraction of molecules having energy equal to or greater than the activation energy at a given temperature is represented by .....