K L Chugh Solutions for Chapter: Chemical Kinetics, Exercise 4: Follow Up Problems

The half life period of a first order reaction is $60$ minutes. What percentage of the reactant will be left behind after $120$ minutes?

A first order reaction is $15\%$ complete in $20$ minutes. In what time will the reaction $60\%$ complete?

The half-life of a first order reaction is $30 \min .$

Calculate the specific rate constant of the reaction.

The half-life of a first order reaction is $30 \min .$

What fraction of the reactant remains after $70 \min ?$

The half-life of a first order reaction is $30 \min .$

How long would be required for $25\%$ of the reactant to be decomposed?

The reaction ${\mathrm{SO}}_2{\mathrm{Cl}}_2\rightleftharpoons {\mathrm{SO}}_2+{\mathrm{Cl}}_2$ is
a first order gas reaction with ${\mathrm{t}}_{1/2}=3.15\times {10}^4 \mathrm{s}$ at $320°\mathrm{C}.$ What percentage of ${\mathrm{SO}}_2{\mathrm{Cl}}_2$ is decomposed on heating this gas for $90$ minutes?

[Hint. Find $\log \frac{\mathrm{a}}{\mathrm{a}-\mathrm{x}}=0.0516$. Now find $\mathrm{x}/\mathrm{a}=0.112$. If $\mathrm{a}=100$ then $\mathrm{x}=100\times 0.112=11.2\%]$

Show that in case of a first order reaction, the time required for $99.9\%$ of the reaction to take place is about ten times than that required for half the reaction.

Half-life of a first order reaction at given temperature is $3$ minutes. Calculate the time required for completion of $3/4\mathrm{th}$ of the reaction.