Embibe Experts Solutions for Chapter: Chemical Kinetics, Exercise 3: EXERCISE-3

For the elementary reaction $2 \mathrm{A}+{\mathrm{B}}_2⟶2\mathrm{AB}$. Calculate how much the rate of reaction will change if the volume of the vessel is reduced to one third of its original volume?

A first order reaction $75\%$ Completed in $72 \min$. How long time will it take for $87.5\%$ completion

Two substance $A$($t_{1/2}=5$ mins$)$ and $B$($t_{1/2}=15$ mins) follow first order kinetics are taken in such a way that initially $\left[\mathrm{A}\right]=4[ \mathrm{B}]$. Calculate the time after which the concentration of both the substance will be equal.

Fill your answer as sum of digits till you get the single digit answer.

For each question, enter the correct numerical value (in decimal notation, truncated/rounded off to the second decimal place; e.g. $6.25, 7.00, -0.33, -.30, 30.27, -127.30$, if answer is 11.36777..... then both $11.36777$..... then both $11.36$ and $11.37$ will be correct) by darken the corresponding bubbles in the ORS.

The specific rate constant for a reaction increases by a factor of 4, if the temperature is change from $27°\mathrm{C}$ to $47°\mathrm{C}$. Find the activation energy for the reaction.

At $380°\mathrm{C}$, the half-life period for the first order decomposition of ${\mathrm{H}}_2{\mathrm{O}}_2$ is $360 \min$. The energy of activation of the reaction is $200 \mathrm{kJ}{ \mathrm{mol}}^{-1}$. Calculate the time required for $75\%$ decomposition at $450°\mathrm{C}$.

A first order reaction, $\mathrm{A}\to \mathrm{B}$, requires activation energy of $70 \mathrm{kJ}{ \mathrm{mol}}^{-1}$. When a $20\%$ solution of $\mathrm{A}$ was kept at $25°\mathrm{C}$ for 20 minutes, $25\%$ decomposition took place. What will be the percent decomposition in the same time in a $30\%$solution maintained at $40°\mathrm{C}$ ? Assume that activation energy remains constant in the same time in a $30\%$ solution maintained at $40°\mathrm{C}$? Assume that activation energy remains constant in this range of temperature.

The reaction $2 \mathrm{A}+\mathrm{B}+\mathrm{C}\to \mathrm{D}+\mathrm{E}$ is found to be first order in $\mathrm{A}$ second in $\mathrm{B}$ and zero order in $\mathrm{C}$. How many times rate increases by increasing concentration of $\mathrm{A},\mathrm{B}$ and $\mathrm{C}$ two times.

The energy of activation of a first order reaction is $104.5 \mathrm{kJ}{ \mathrm{mol}}^{-1}$ and pre-exponential factor (A) is $5\times {10}^{13}{\sec }^{-1}$. At what temperature, will the reaction have a half life of 1 minute?