(A) The rate law for the reaction is given by: $\text{Rate} = k[A]^1[B]^2[C]^0$. When the concentration of all reactants is doubled,the new concentrat

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Rate of reaction increases $8$ times.

(A) The rate law for the reaction is given by: $\text{Rate} = k[A]^1[B]^2[C]^0$. When the concentration of all reactants is doubled,the new concentrations are $[A]' = 2[A]$,$[B]' = 2[B]$,and $[C]' = 2[C]$. The new rate $(\text{Rate})_1$ is: $(\text{Rate})_1 = k[2A]^1[2B]^2[2C]^0$. $(\text{Rate})_1 = k \times 2[A] \times 4[B]^2 \times 1$. $(\text{Rate})_1 = 8 \times k[A][B]^2$. Therefore,the rate of reaction increases $8$ times.

Class 12 Chemistry Chemical Kinetics Rate law , Rate constant , Order of Reaction and Molecularity

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The reaction $2 A + B + C \longrightarrow D + E$ is found to be first order in $A$,second order in $B$,and zero order in $C$. What is the effect of increasing the concentration of all reactants twice?

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A
Rate of reaction increases $8$ times.
B
Rate of reaction increases $24$ times.
C
Rate of reaction increases $36$ times.
D
Rate of reaction remains unaffected.

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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The rate of the reaction $x + y \rightarrow \text{product}$ is $5.4 \times 10^{-2} \ mol \ dm^{-3} \ sec^{-1}$. When $[x] = 0.2 \ mol \ dm^{-3}$ and $[y] = 0.1 \ mol \ dm^{-3}$,calculate the rate constant of the reaction if it is first order in $X$ and second order in $Y$.

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The mechanism of the reaction $A + 2B \to D$ is given by:
$2B \xrightarrow{k} B_2$ [Slow]
$B_2 + A \to D$ [Fast]
The rate law expression,order with respect to $A$,order with respect to $B$,and overall order are respectively:

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Which of the following statements is incorrect?

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If the rate expression for a chemical reaction is given by $\text{Rate} = k[A]^m[B]^n$,what is the order of the reaction?

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At a certain temperature,the half-life periods for the catalytic decomposition of $NH_3$ were found to be as follows:

Pressure $(mm \ Hg)$ $50, 100, 200$

Half-life period $(hrs)$ $3.52, 1.76, 0.88$

What will be the pressure when the half-life period is $2.5 \ hrs$?

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Pressure $(mm \ Hg)$	$50, 100, 200$
Half-life period $(hrs)$	$3.52, 1.76, 0.88$

The reaction $2 A + B + C \longrightarrow D + E$ is found to be first order in $A$,second order in $B$,and zero order in $C$. What is the effect of increasing the concentration of all reactants twice?

Similar Questions

The rate of the reaction $x + y \rightarrow \text{product}$ is $5.4 \times 10^{-2} \ mol \ dm^{-3} \ sec^{-1}$. When $[x] = 0.2 \ mol \ dm^{-3}$ and $[y] = 0.1 \ mol \ dm^{-3}$,calculate the rate constant of the reaction if it is first order in $X$ and second order in $Y$.

The mechanism of the reaction $A + 2B \to D$ is given by:$2B \xrightarrow{k} B_2$ [Slow]$B_2 + A \to D$ [Fast]The rate law expression,order with respect to $A$,order with respect to $B$,and overall order are respectively:

Which of the following statements is incorrect?

If the rate expression for a chemical reaction is given by $\text{Rate} = k[A]^m[B]^n$,what is the order of the reaction?

At a certain temperature,the half-life periods for the catalytic decomposition of $NH_3$ were found to be as follows: Pressure $(mm \ Hg)$ $50, 100, 200$ Half-life period $(hrs)$ $3.52, 1.76, 0.88$ What will be the pressure when the half-life period is $2.5 \ hrs$?

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The mechanism of the reaction $A + 2B \to D$ is given by:
$2B \xrightarrow{k} B_2$ [Slow]
$B_2 + A \to D$ [Fast]
The rate law expression,order with respect to $A$,order with respect to $B$,and overall order are respectively:

At a certain temperature,the half-life periods for the catalytic decomposition of $NH_3$ were found to be as follows:

Pressure $(mm \ Hg)$ $50, 100, 200$

Half-life period $(hrs)$ $3.52, 1.76, 0.88$

What will be the pressure when the half-life period is $2.5 \ hrs$?