(A) The rate law for the reaction is given by $Rate = k[A]^x[B]^y$. From the first condition,when $[A]$ is doubled,the rate doubles: $2 \times Rate =

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(A) The rate law for the reaction is given by $Rate = k[A]^x[B]^y$. From the first condition,when $[A]$ is doubled,the rate doubles: $2 \times Rate = k[2A]^x[B]^y$. This implies $2^x = 2$,so $x = 1$. From the second condition,when both $[A]$ and $[B]$ are doubled,the rate becomes four times: $4 \times Rate = k[2A]^x[2B]^y$. Substituting $x = 1$: $4 \times Rate = k[2A]^1[2B]^y = 2 \times 2^y \times k[A][B]^y$. $4 = 2 \times 2^y$,which means $2 = 2^y$,so $y = 1$. Thus,the order with respect to $A$ is $1$ and with respect to $B$ is $1$.

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

Medium

For a reaction $A + B \rightarrow \text{Product}$,the rate of reaction doubles when the concentration of $A$ is doubled. The rate becomes four times when the concentrations of both $A$ and $B$ are doubled. What is the order of the reaction with respect to $A$ and $B$ respectively?

A
$1, 1$
B
$2, 0$
C
$1, 0$
D
$0, 1$

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

For the reaction $2N_2O_5 \to 4NO_2 + O_2$,the rate of reaction and rate constant are $1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$ and $3.4 \times 10^{-5} \ s^{-1}$ respectively. The concentration of $N_2O_5$ at that time will be:

Medium

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The rate constant for the reaction,$2N_2O_5 \to 4NO_2 + O_2$ is $3 \times 10^{-5} \, s^{-1}$. If the rate is $2.40 \times 10^{-5} \, mol \, L^{-1} \, s^{-1}$,then the concentration of $N_2O_5$ (in $mol \, L^{-1}$) is

MediumIIT 2000

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From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant.
$(i)$ $3 NO_{(g)} \rightarrow N_2O_{(g)}$ Rate $= k[NO]^2$

Medium

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The reaction $N_2O_5$ (in $CCl_4$ solution) $\to 2NO_2$ (solution) $+ \frac{1}{2}O_{2(g)}$ is of first order in $N_2O_5$ with rate constant $6.2 \times 10^{-1} \, s^{-1}$. What is the value of the rate of reaction when $[N_2O_5] = 1.25 \, mol \, L^{-1}$?

Easy

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Write the formula for the rate of reaction $R \to P$ for zero-order and first-order reactions.

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For a reaction $A + B \rightarrow \text{Product}$,the rate of reaction doubles when the concentration of $A$ is doubled. The rate becomes four times when the concentrations of both $A$ and $B$ are doubled. What is the order of the reaction with respect to $A$ and $B$ respectively?

Similar Questions

For the reaction $2N_2O_5 \to 4NO_2 + O_2$,the rate of reaction and rate constant are $1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$ and $3.4 \times 10^{-5} \ s^{-1}$ respectively. The concentration of $N_2O_5$ at that time will be:

The rate constant for the reaction,$2N_2O_5 \to 4NO_2 + O_2$ is $3 \times 10^{-5} \, s^{-1}$. If the rate is $2.40 \times 10^{-5} \, mol \, L^{-1} \, s^{-1}$,then the concentration of $N_2O_5$ (in $mol \, L^{-1}$) is

From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant.$(i)$ $3 NO_{(g)} \rightarrow N_2O_{(g)}$ Rate $= k[NO]^2$

The reaction $N_2O_5$ (in $CCl_4$ solution) $\to 2NO_2$ (solution) $+ \frac{1}{2}O_{2(g)}$ is of first order in $N_2O_5$ with rate constant $6.2 \times 10^{-1} \, s^{-1}$. What is the value of the rate of reaction when $[N_2O_5] = 1.25 \, mol \, L^{-1}$?

Write the formula for the rate of reaction $R \to P$ for zero-order and first-order reactions.

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From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant.
$(i)$ $3 NO_{(g)} \rightarrow N_2O_{(g)}$ Rate $= k[NO]^2$