JEE Main Chemical Kinetics and Nuclear Chemistry Practice Questions With Solutions

For a reaction $A\stackrel{{\mathrm{K}}_1}{\to }\mathrm{B}\stackrel{{\mathrm{K}}_2}{\to }\mathrm{C}$A \overset{K_{1} }{\rightarrow} \textrm{ } B \overset{K_{2} }{\rightarrow} CIf the rate of formation of B is set to be zero then the concentration of B is given by :

Integrated rate law equation for a first order gas phase reaction is given by (where ${\mathrm{P}}_{\mathrm{i}}$P_{i} is initial pressure and ${\mathrm{P}}_{\mathrm{t}}$P_{t} is total pressure at time $t$t)

For a chemical reaction $\mathrm{A}+\mathrm{B}\to$A + B \rightarrow Product, the order is 1 with respect to $\mathrm{A}$A and $\mathrm{B}$B.

What is the value of $x$x and $y$y ?

The correct reaction profile diagram for a positive catalyst reaction.

Consider the following reaction that goes from A to B in three steps as shown below:

Choose the correct option

A student has studied the decomposition of a gas AB${}_3$_{3} at 25${}^{\circ }$^{\circ}C. He obtained the following data.

The order of the reaction is

For kinetic study of the reaction of iodide ion with ${\mathrm{H}}_2{\mathrm{O}}_2$H_{2} O_{2} at room temperature :

(A) Always use freshly prepared starch solution.

(B) Always keep the concentration of sodium thiosulphate solution less than that of KI solution.

(C) Record the time immediately after the appearance of blue colour.

(D) Record the time immediately before the appearance of blue colour.

(E) Always keep the concentration of sodium thiosulphate solution more than that of KI solution.

Choose the correct answer from the options given below :

At ${30}^{\circ }\mathrm{C}$30^{\circ} C, the half life for the decomposition of ${\mathrm{AB}}_2$AB_{2} is $200\mathrm{s}$200 \textrm{ } s and is independent of the initial concentration of ${\mathrm{AB}}_2$AB_{2}. The time required for $80\mathrm{\%}$80 \% of the ${\mathrm{AB}}_2$AB_{2} to decompose is

Given: $\log 2=0.30$log ⁡ 2 = 0.30$\log 3=0.48$log ⁡ 3 = 0.48

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' is

(Given : ln 10 = 2.303 and log 2 = 0.3010)