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

For a first order reaction,the slope of the graph of $\log_{10}[A]_t$ versus time is equal to:

What is the half-life of a first-order reaction if the time required to decrease the concentration of the reactant from $0.8 \ mol \ dm^{-3}$ to $0.2 \ mol \ dm^{-3}$ is $12 \ hour$ (in $hour$)?

$A_{(g)} \rightarrow B_{(g)} + C_{(g)}$ 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 $k$?

For the first-order gaseous reaction $A \rightarrow 2B + C$ at $373 \, K$,starting with pure $A$,the total pressure of the system after $10 \, min$ is $176 \, mm \, Hg$ and after a long time,it is $270 \, mm \, Hg$. Based on this information,calculate: $(1)$ Initial pressure of $A$,$(2)$ Pressure of $A$ after $10 \, min$,and $(3)$ Rate constant.

For a first-order reaction,the concentration decreases from $800 \ mol/dm^3$ to $50 \ mol/dm^3$ in $2 \times 10^4 \ s$. What is the rate constant of the reaction?