The rate of first order reaction is 1.5*10^-2 molL-1/min-1 at 0.5 m .c

1.	The rate of first order reaction is 1.5*10^-2 molL-1/min-1 at 0.5 m .concentration of the reactant .the half life of the reaction is
Answer» Answer : The half life of the reaction is, 23.1 minutes. Solution : GIVEN, RATE of first ORDER reaction = $1.5\times 10^{-2}molL^{-1}min^{-1}$ Concentration of reactant = 0.5 m = 0.5 mole/L For first order reaction, $A\rightarrow Product$ The expression for rate of reaction is, $r=K[A]\\K=\frac{r}{[A]}$ Now put all the given values in this formula, we get the value for rate constant. $K=\frac{1.5\times 10^{-2}mol L^{-1} min^{-1}}{0.5mole/L}=3\times 10^{-2}min^{-1}$ The formula for half life for first order reaction is, $t_{1/2}=\frac{0.693}{K}$ Now put the value of K, we get the value of half life. $t_{1/2}=\frac{0.693}{3\times 10^{-2}min^{-1}}=23.1min$ Therefore, the half life of the reaction is, 23.1 minutes.