320189 The rate expression for the reaction \({\rm{A(g) + B(g)}} \to {\rm{C(g)}}\) is rate \(=\mathrm{k}[\mathrm{A}][\mathrm{B}]^{-1}\).

What changes in the initial concentrations of A and B will cause the rate of reaction to decrease by a factor of half?

320190 The rate law for a reaction between the
substances \(\mathrm{A}\) and \(\mathrm{B}\) is given by
Rate \(=\mathrm{k}[\mathrm{A}]^{\mathrm{n}}[\mathrm{B}]^{\mathrm{m}}\)
On doubling the concentration of A and halving
the concentration of \(B\), the ratio of the new rate
to the earlier rate of the reaction will be as

320191 The chemical reaction \(2 \mathrm{O}_{3} \longrightarrow 3 \mathrm{O}_{2}\) proceeds as
follows:
\(\mathrm{O}_{3} \xrightarrow{\text { Fast }} \mathrm{O}_{2}+\mathrm{O} ; \quad \mathrm{O}+\mathrm{O}_{3} \xrightarrow{\text { Slow }} 2 \mathrm{O}_{2}\)
the rate law expression should be

320192 The reaction \({\text{2NO(g)}} + {{\text{O}}_{\text{2}}}{\text{(g)}} \rightleftharpoons {\text{2N}}{{\text{O}}_{\text{2}}}{\text{(g)}}\) is of first order. If volume of reaction vessel is reduced to \(1 / 3\) the rate of reaction would be

320189 The rate expression for the reaction \({\rm{A(g) + B(g)}} \to {\rm{C(g)}}\) is rate \(=\mathrm{k}[\mathrm{A}][\mathrm{B}]^{-1}\).

What changes in the initial concentrations of A and B will cause the rate of reaction to decrease by a factor of half?

320190 The rate law for a reaction between the
substances \(\mathrm{A}\) and \(\mathrm{B}\) is given by
Rate \(=\mathrm{k}[\mathrm{A}]^{\mathrm{n}}[\mathrm{B}]^{\mathrm{m}}\)
On doubling the concentration of A and halving
the concentration of \(B\), the ratio of the new rate
to the earlier rate of the reaction will be as

320191 The chemical reaction \(2 \mathrm{O}_{3} \longrightarrow 3 \mathrm{O}_{2}\) proceeds as
follows:
\(\mathrm{O}_{3} \xrightarrow{\text { Fast }} \mathrm{O}_{2}+\mathrm{O} ; \quad \mathrm{O}+\mathrm{O}_{3} \xrightarrow{\text { Slow }} 2 \mathrm{O}_{2}\)
the rate law expression should be

320192 The reaction \({\text{2NO(g)}} + {{\text{O}}_{\text{2}}}{\text{(g)}} \rightleftharpoons {\text{2N}}{{\text{O}}_{\text{2}}}{\text{(g)}}\) is of first order. If volume of reaction vessel is reduced to \(1 / 3\) the rate of reaction would be

320189 The rate expression for the reaction \({\rm{A(g) + B(g)}} \to {\rm{C(g)}}\) is rate \(=\mathrm{k}[\mathrm{A}][\mathrm{B}]^{-1}\).

What changes in the initial concentrations of A and B will cause the rate of reaction to decrease by a factor of half?

320190 The rate law for a reaction between the
substances \(\mathrm{A}\) and \(\mathrm{B}\) is given by
Rate \(=\mathrm{k}[\mathrm{A}]^{\mathrm{n}}[\mathrm{B}]^{\mathrm{m}}\)
On doubling the concentration of A and halving
the concentration of \(B\), the ratio of the new rate
to the earlier rate of the reaction will be as

320191 The chemical reaction \(2 \mathrm{O}_{3} \longrightarrow 3 \mathrm{O}_{2}\) proceeds as
follows:
\(\mathrm{O}_{3} \xrightarrow{\text { Fast }} \mathrm{O}_{2}+\mathrm{O} ; \quad \mathrm{O}+\mathrm{O}_{3} \xrightarrow{\text { Slow }} 2 \mathrm{O}_{2}\)
the rate law expression should be

320192 The reaction \({\text{2NO(g)}} + {{\text{O}}_{\text{2}}}{\text{(g)}} \rightleftharpoons {\text{2N}}{{\text{O}}_{\text{2}}}{\text{(g)}}\) is of first order. If volume of reaction vessel is reduced to \(1 / 3\) the rate of reaction would be

320189 The rate expression for the reaction \({\rm{A(g) + B(g)}} \to {\rm{C(g)}}\) is rate \(=\mathrm{k}[\mathrm{A}][\mathrm{B}]^{-1}\).

What changes in the initial concentrations of A and B will cause the rate of reaction to decrease by a factor of half?

320190 The rate law for a reaction between the
substances \(\mathrm{A}\) and \(\mathrm{B}\) is given by
Rate \(=\mathrm{k}[\mathrm{A}]^{\mathrm{n}}[\mathrm{B}]^{\mathrm{m}}\)
On doubling the concentration of A and halving
the concentration of \(B\), the ratio of the new rate
to the earlier rate of the reaction will be as

320191 The chemical reaction \(2 \mathrm{O}_{3} \longrightarrow 3 \mathrm{O}_{2}\) proceeds as
follows:
\(\mathrm{O}_{3} \xrightarrow{\text { Fast }} \mathrm{O}_{2}+\mathrm{O} ; \quad \mathrm{O}+\mathrm{O}_{3} \xrightarrow{\text { Slow }} 2 \mathrm{O}_{2}\)
the rate law expression should be

320192 The reaction \({\text{2NO(g)}} + {{\text{O}}_{\text{2}}}{\text{(g)}} \rightleftharpoons {\text{2N}}{{\text{O}}_{\text{2}}}{\text{(g)}}\) is of first order. If volume of reaction vessel is reduced to \(1 / 3\) the rate of reaction would be