Consider the two different first order reactions given below

$$\begin{aligned} & \mathrm{A}+\mathrm{B} \rightarrow \mathrm{C} \text { (Reaction 1) } \\ & \mathrm{P} \rightarrow \mathrm{Q} \text { (Reaction 2) } \end{aligned}$$

The ratio of the half life of Reaction 1 : Reaction 2 is $5: 2$ If $t_1$ and $t_2$ represent the time taken to complete $2 / 3^{\text {rd }}$ and $4 / 5^{\text {th }}$ of Reaction 1 and Reaction 2 , respectively, then the value of the ratio $t_1: t_2$ is _________ $\times 10^{-1}$ (nearest integer). [Given : $\log _{10}(3)=0.477$ and $\log _{10}(5)=0.699$]

For a first order reaction, the time required for completion of 90% reaction is 'x' times the half life of the reaction. The value of 'x'…

During Kinetic study of reaction $\mathrm{2 A+B \rightarrow C+D}$, the following results were obtained : .tg…

If compound A reacts with B following first order kinetics with rate constant $2.011 \times 10^{-3} \mathrm{~s}^{-1}$. The time taken by…

A $\to$ B The rate constants of the above reaction at 200 K and 300 K are 0.03 min$^{-1}$ and 0.05 min$^{-1}$ respectively. The activation…

$$2 \mathrm{NO}+2 \mathrm{H}_{2} \rightarrow \mathrm{N}_{2}+2 \mathrm{H}_{2} \mathrm{O}$$ The above reaction has been studied at…