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Q.
The rate for a first order reaction is $0.693 \times 10^{-2} mol L^{-1}
min^{-1}$ and the initial concentration of the reactants is $1M,
t_{1/2}$ is equal to
Chemical Kinetics
Solution:
$r=k\left[reactant\right]^{-1}$
$\therefore k=\frac{0.693\times10^{-2}}{1}$
also $t_{12}=\frac{0.693}{k}=\frac{0.693}{0.693\times10^{-2}}=100 \,min$