(C) The rate of appearance of $B$ is determined by the first reaction path.For the reaction $A \rightarrow 2B$,the rate of reaction is given by $\frac

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$8 \times 10^{-3} \ M \ s^{-1}$

(C) The rate of appearance of $B$ is determined by the first reaction path.For the reaction $A \rightarrow 2B$,the rate of reaction is given by $\frac{1}{2} \frac{d[B]}{dt} = K_1 [A]$.Therefore,$\frac{d[B]}{dt} = 2 K_1 [A]$.Given $K_1 = 2 \times 10^{-3} \ s^{-1}$ and $[A] = 2 \ M$.$\frac{d[B]}{dt} = 2 \times (2 \times 10^{-3} \ s^{-1}) \times (2 \ M) = 8 \times 10^{-3} \ M \ s^{-1}$.

Class 12 Chemistry Chemical Kinetics Rate of a reaction

Medium

For the decomposition of $A$ as shown below,calculate the rate of appearance of $B$ if the initial concentration of $A$ is $2 \ M$.
$A_{(g)} \xrightarrow{K_1 = 2 \times 10^{-3} \ s^{-1}} 2B_{(g)}$
$A_{(g)} \xrightarrow{K_2 = 1 \times 10^{-3} \ s^{-1}} C_{(g)}$

A
$2 \times 10^{-3} \ M \ s^{-1}$
B
$4 \times 10^{-3} \ M \ s^{-1}$
C
$8 \times 10^{-3} \ M \ s^{-1}$
D
None of these

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In a catalytic conversion of $N_2$ to $NH_3$ by Haber's process,the rate of reaction was expressed as change in the concentration of ammonia per time is $40 \times 10^{-3} \ mol \ L^{-1} s^{-1}$. If there are no side reactions,the rate of the reaction as expressed in terms of hydrogen is (in $mol \ L^{-1} s^{-1}$)

Medium

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For the reaction $2N_2O_{5(g)} \rightleftharpoons 4NO_{2(g)} + O_{2(g)}$ in a closed vessel,the concentration of $NO_2$ increases by $2.0 \times 10^{-2} \, mol \, L^{-1}$ in $5 \, s$. Calculate the rate of reaction.

Medium

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Consider the following reaction: $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$. The rate of this reaction in terms of $N_2$ at $T \ K$ is $\frac{-d[N_2]}{dt} = 0.02 \ mol \ L^{-1} \ s^{-1}$. What is the value of $\frac{-d[H_2]}{dt}$ (in units of $mol \ L^{-1} \ s^{-1}$) at the same temperature?

MediumTS EAMCET 2002

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The concentration of a reactant decreases from $0.2 \ M$ to $0.1 \ M$ in $10 \ \text{minutes}$. The rate of the reaction is

Easy

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Thermal decomposition of $N_2O_5$ occurs as per the equation below:
$2N_2O_5 \longrightarrow 4NO_2 + O_2$
The correct statement is:

DifficultKVPY 2019

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For the decomposition of $A$ as shown below,calculate the rate of appearance of $B$ if the initial concentration of $A$ is $2 \ M$.$A_{(g)} \xrightarrow{K_1 = 2 \times 10^{-3} \ s^{-1}} 2B_{(g)}$$A_{(g)} \xrightarrow{K_2 = 1 \times 10^{-3} \ s^{-1}} C_{(g)}$

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For the reaction $2N_2O_{5(g)} \rightleftharpoons 4NO_{2(g)} + O_{2(g)}$ in a closed vessel,the concentration of $NO_2$ increases by $2.0 \times 10^{-2} \, mol \, L^{-1}$ in $5 \, s$. Calculate the rate of reaction.

Consider the following reaction: $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$. The rate of this reaction in terms of $N_2$ at $T \ K$ is $\frac{-d[N_2]}{dt} = 0.02 \ mol \ L^{-1} \ s^{-1}$. What is the value of $\frac{-d[H_2]}{dt}$ (in units of $mol \ L^{-1} \ s^{-1}$) at the same temperature?

The concentration of a reactant decreases from $0.2 \ M$ to $0.1 \ M$ in $10 \ \text{minutes}$. The rate of the reaction is

Thermal decomposition of $N_2O_5$ occurs as per the equation below:$2N_2O_5 \longrightarrow 4NO_2 + O_2$The correct statement is:

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For the decomposition of $A$ as shown below,calculate the rate of appearance of $B$ if the initial concentration of $A$ is $2 \ M$.
$A_{(g)} \xrightarrow{K_1 = 2 \times 10^{-3} \ s^{-1}} 2B_{(g)}$
$A_{(g)} \xrightarrow{K_2 = 1 \times 10^{-3} \ s^{-1}} C_{(g)}$

Thermal decomposition of $N_2O_5$ occurs as per the equation below:
$2N_2O_5 \longrightarrow 4NO_2 + O_2$
The correct statement is: