In a first-order reaction,the concentration of the reactant decreases from $0.80 \, mol \, L^{-1}$ to $0.06 \, mol \, L^{-1}$ in $45 \, min$. Calculate the half-life $(t_{1/2})$. (in $, min$)

The reaction $A \rightarrow B$ follows first-order kinetics. If it takes $1 \text{ hour}$ to convert $0.8 \text{ mol}$ of $A$ to $0.6 \text{ mol}$ of $B$,how many hours will it take to convert $0.9 \text{ mol}$ of $A$ to $0.675 \text{ mol}$ of $B$?

For a first order reaction,the rate constant is given as $\log_{10} K = 12 - \frac{6 \times 10^3}{T}$. What will be the value of temperature if its half-life period is $6.93 \times 10^{-3} \, \text{min}$ (in $, K$)?

The plot of $\log(a - x)$ versus time $t$ is a straight line,which indicates that the reaction is of ....... order.

What is the numerical value of the rate constant of a first-order reaction that is $20 \%$ completed in $10 \ min$ (in $min^{-1}$)?

For a first order gas phase elementary reaction $A_{(g)} \xrightarrow{k} 2B_{(g)}$,which of the following is $INCORRECT$?