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:

Two substances $\mathrm{R}$ and $\mathrm{S}$ decompose in a solution independently, both following first order kinetics. The rate constant of $\mathrm{R}$ is twice that of $\mathrm{S}.$ In an experiment, the solution initially contained $0.5$ millimoles of $\mathrm{R}$ and $0.25$ millimoles of $\mathrm{S}.$ The molarities of $\mathrm{R}$ and $\mathrm{S}$ will be equal just at the end of time equal to:

Consider the water gas equilibrium reaction,

$\mathrm{C}\left(\mathrm{s}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{CO}\left(\mathrm{g}\right)+{\mathrm{H}}_2\left(\mathrm{g}\right)$

Which of the following statements is true at equilibrium?

A drop of a solution (volume$=0.05 \mathrm{ml})$ contains $6\times {10}^{-7} \mathrm{mol}$ of ${\mathrm{H}}^{+}.$ If the rate of disappearance of ${\mathrm{H}}^{+}$ is $6.0\times {10}^5 \mathrm{mol} {\mathrm{lit}}^{-1}{\mathrm{s}}^{-1},$ how long will it take for the ${\mathrm{H}}^{+}$ in the drop to disappear?

The rate expression for the reaction $\mathrm{A}\left(\mathrm{g}\right)+\mathrm{B}\left(\mathrm{g}\right)\to \mathrm{C}\left(\mathrm{g}\right)$ is $\mathrm{k} {\mathrm{C}}_{\mathrm{A}}^{2 } {\mathrm{C}}_{\mathrm{B}}^{1/4}.$ What changes in the initial concentrations of $\mathrm{A}$ and $\mathrm{B}$ will cause the rate of reaction to increase by a factor of eight?