In a first order reaction,the concentration of the reactant is reduced from $0.6 \ mol \ L^{-1}$ to $0.2 \ mol \ L^{-1}$ in $5 \ min$. What is the rate constant of the reaction (in $min^{-1}$)? $(\log 3 = 0.4771)$

For a first order reaction $A \to B$,the reaction rate at reactant concentration of $0.01 \ M$ is found to be $2.0 \times 10^{-5} \ mol \ L^{-1} \ s^{-1}$. The half-life period of the reaction is .......... $sec$.

When the value of rate constant $(k)$ is $2.0 \text{ min}^{-1}$,then what will be the half-life of the reaction $(t_{1/2})$ in seconds?

$A_{(g)} \rightarrow B_{(g)} + C_{(g)}$ is a first order reaction.

Time	$t$	$\infty$
$P_{\text{system}}$	$P_t$	$P_{\infty}$

The reaction was started with reactant $A$ only. Which of the following expressions is correct for the rate constant $k$?

The half-life period for a first-order reaction is . . . . . . .

The half-life for the decomposition of gaseous compound $A$ is $240 \ s$ when the initial gaseous pressure is $500 \ Torr$. When the initial pressure is $250 \ Torr$,the half-life is found to be $4.0 \ min$. The order of the reaction is....... (Nearest integer)