For a reaction, A $$\to$$ B, enthalpy of reaction is $$-$$4.2 kJ mol^$$-$$1 and enthalpy of activation is 9.6 kJ mol^$$-$$1. The correct potential energy profile for the reaction is shown in option.

The slope of Arrhenius plot $$\left( {\ln \,k\,v/s{1 \over T}} \right)$$ of first order reactino is $$-$$5 $$\times$$ 10³K. The value of E_a of the reaction is. Choose the correct option for your answer.

[Given R = 8.314 JK^$$-$$1mol^$$-$$1]

An increase in the concentration of the reactants of a reaction leads to change in :

The rate constant for a first order reaction is 4.606 $$ \times $$ 10^-3 s^-1. The time required to reduce 2.0 g of the reactant to 0.2 g is :