(B) The initial rate is $r_1 = K[x][y]$.When the volume of the vessel is reduced to $1/4$ of its initial volume $(V_2 = V_1/4)$,the concentration of t

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(B) The initial rate is $r_1 = K[x][y]$.When the volume of the vessel is reduced to $1/4$ of its initial volume $(V_2 = V_1/4)$,the concentration of the reactants increases by a factor of $4$ because concentration $C = n/V$.Therefore,the new concentrations are $[x]_2 = 4[x]$ and $[y]_2 = 4[y]$.The new rate $r_2 = K[x]_2[y]_2 = K(4[x])(4[y]) = 16K[x][y]$.Thus,$r_2 = 16r_1$.The rate of the reaction increases by $16$ times.

Class 12 Chemistry Chemical Kinetics Rate of a reaction

Medium

The rate of a gaseous reaction is given by $r = K[x][y]$. If the volume of the reaction vessel is suddenly reduced to $1/4$ of its initial volume,the rate of the reaction will ............

A
increase by $1/8$ times
B
increase by $16$ times
C
remain constant
D
increase or decrease

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Chemical Kinetics

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Rate of a reaction

For the reaction $R \rightarrow P$,the concentration of a reactant changes from $0.03 \, M$ to $0.02 \, M$ in $25 \, minutes$. Calculate the average rate of reaction using units of time both in $minutes$ and $seconds$.

Difficult

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The instantaneous rate for the reaction $2 A + B \rightarrow C + 3 D$ is given by:

EasyMHT CET 2022

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For a reaction,$2 \ N_2O_{5(g)} \longrightarrow 4 \ NO_{2(g)} + O_{2(g)}$. The $N_2O_5$ disappears at a rate of $0.06 \ mol \ dm^{-3} \ s^{-1}$. What is the rate of $NO_{2(g)}$ formation (in $mol \ dm^{-3} \ s^{-1}$)?

MediumMHT CET 2024

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For the reaction $2A + 3B \rightarrow 4C$,the rate of reaction is expressed as:

Easy

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Consider the reaction: $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$. The equality relationship between $\frac{d[NH_3]}{dt}$ and $\frac{d[H_2]}{dt}$ is

MediumAIPMT 2006

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The rate of a gaseous reaction is given by $r = K[x][y]$. If the volume of the reaction vessel is suddenly reduced to $1/4$ of its initial volume,the rate of the reaction will ............

Similar Questions

For the reaction $R \rightarrow P$,the concentration of a reactant changes from $0.03 \, M$ to $0.02 \, M$ in $25 \, minutes$. Calculate the average rate of reaction using units of time both in $minutes$ and $seconds$.

The instantaneous rate for the reaction $2 A + B \rightarrow C + 3 D$ is given by:

For a reaction,$2 \ N_2O_{5(g)} \longrightarrow 4 \ NO_{2(g)} + O_{2(g)}$. The $N_2O_5$ disappears at a rate of $0.06 \ mol \ dm^{-3} \ s^{-1}$. What is the rate of $NO_{2(g)}$ formation (in $mol \ dm^{-3} \ s^{-1}$)?

For the reaction $2A + 3B \rightarrow 4C$,the rate of reaction is expressed as:

Consider the reaction: $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$. The equality relationship between $\frac{d[NH_3]}{dt}$ and $\frac{d[H_2]}{dt}$ is

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