Question

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 1

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.

Answer 2

Answer:23.1 min

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