$A \rightarrow P$ is a zero order reaction. At 298 K the rate constant of the reaction is $1 \times 10^{-3} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$. Initial concentration of ' $A$ ' is $0.1 \mathrm{~mol} \mathrm{~L}^{-1}$. What is the concentration of ' $A$ after 10 sec ?

The rate constant of a first order reaction is $3.46 \times 10^{-2} \mathrm{~s}^{-1}$ at 298 K . What is the rate constant of the reaction at 350 K if its activation energy is $50.1 \mathrm{~kJ} \mathrm{~mol}^{-1}$, $\left(R=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)(\log 2=0.3010)$

At 298 K the value of $-\frac{\Delta\left[\mathrm{Br}^{-}\right]}{\Delta t}$ for the reaction,

$5 \mathrm{Br}^{-}(a q)+\mathrm{BrO}_3^{-}(a q)+6 \mathrm{H}^{+}(a q) \longrightarrow 3 \mathrm{Br}_2(a q)+3 \mathrm{H}_2 \mathrm{O}(l)$ is $X$ $\mathrm{mol} \mathrm{L} \mathrm{min}^{-1}$. What is the rate (in $\mathrm{mol} \mathrm{L}^{-1} \mathrm{~min}^{-1}$ ) of this reaction?