The equilibrium that remains unaffected by pressure change is:

The catalyst iron employed in the Haber's process contains molybdenum, the function of which is

The rate constant of a reaction at temperature $200 \mathrm{K}$ is $10$ times less than the rate constant at $400 \mathrm{K}.$ What is the activation energy of the reaction?

The rate constant for forward reaction and backward reaction of the hydrolysis of ester are $1.1\times {10}^{-2}$ and $1.5\times {10}^{-3}$ per minute respectively. Equilibrium constant for the reaction is ${\mathrm{CH}}_3{\mathrm{COOC}}_2{\mathrm{H}}_5+{\mathrm{H}}_2\mathrm{O}\rightleftharpoons {\mathrm{CH}}_3\mathrm{COOH}+{\mathrm{C}}_2{\mathrm{H}}_5\mathrm{OH}$:

The equilibrium $2{\mathrm{SO}}_{2( \mathrm{g})}+{\mathrm{O}}_{2( \mathrm{g})}\rightleftharpoons 2{\mathrm{SO}}_{3( \mathrm{g})}$ shifts forward if:

For the system, $3\mathrm{A}+2\mathrm{B}\rightleftharpoons 2\mathrm{C},$ the expression for equilibrium constant $\mathrm{K}$ is:

The time taken for $90\%$ of a first order reaction to complete is approximately:

The rate law for a reaction between the substances $\mathrm{A}$ and $\mathrm{B}$ is given by Rate$=\mathrm{k}\left[\mathrm{A}{]}^{\mathrm{n}}\right[\mathrm{B}{]}^{\mathrm{m}}$.

On doubling the concentration of $\mathrm{A}$ and halving the concentration of $\mathrm{B},$ the ratio of the new rate to the earlier rate of the reaction will be as:

The following data are for the decomposition of ammonium nitrite in aqueous solution,

The order of reaction is: