If benzene diazonium chloride undergoes first order decomposition at $T(\mathrm{~K})$ with a rate constant of $6.93 \times 10^{-2} \mathrm{~min}^{-1}$, the time for completion of $90 \%$ of the reaction (in min ) is (nearest integer) $(\log 2=0.30$, $\log 3=0.477$ )

For a reaction, the threshold energy is $75 \mathrm{~kJ} /$ mole. If the internal energy of the reactants is 20 $\mathrm{kJ} /$ mole, the activation energy (in $\mathrm{kJ} /$ mole) is

145. Rate constants in the following reaction are Reaction 1 :

$$ A \xrightarrow{\text { Catalyst } 1} P_1, k_1=1 \mathrm{~s}^{-1} $$

Reaction 2 :

$$ A \xrightarrow{\text { Catalyst } 2} P_2, k_2=0.1 \mathrm{~L} \mathrm{~mol}^{-1} \mathrm{~s}^{-1} $$

Reaction 3 :

$$ A \xrightarrow{\text { Catalyst } 3} P_3, k_3=0.01 \mathrm{~L} \mathrm{~mol}^{-1} \mathrm{~s}^{-1} $$

The correct relations between the rate of the reactions at 1 M of $A$ are

Which of the following is a zero order reaction?