(B) The given reaction is $2A + B \longrightarrow 2C$. According to the rate law expression for the reaction: $-\frac{1}{2} \frac{d[A]}{dt} = -\frac{d

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(B) The given reaction is $2A + B \longrightarrow 2C$. According to the rate law expression for the reaction: $-\frac{1}{2} \frac{d[A]}{dt} = -\frac{d[B]}{dt} = \frac{1}{2} \frac{d[C]}{dt}$. Given that the rate of disappearance of $A$ is $-\frac{d[A]}{dt} = 0.076 \ mol \ s^{-1}$. Substituting this into the rate expression: $-\frac{d[B]}{dt} = \frac{1}{2} \times (-\frac{d[A]}{dt}) = \frac{1}{2} \times 0.076 \ mol \ s^{-1} = 0.038 \ mol \ s^{-1}$. Therefore,the rate of disappearance of $B$ is $0.038 \ mol \ s^{-1}$.

Class 12 Chemistry Chemical Kinetics Rate of a reaction

Medium

For the reaction $2A + B \rightarrow 2C$,the rate of disappearance of $A$ is $0.076 \ mol \ s^{-1}$. What is the rate of disappearance of $B$?

MHT CET 2021 All MHT CET

A
$0.076 \ mol \ s^{-1}$
B
$0.038 \ mol \ s^{-1}$
C
$0.019 \ mol \ s^{-1}$
D
$0.095 \ mol \ s^{-1}$

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For the chemical reaction $N_2 + 3H_2 \rightarrow 2NH_3$,the rate of reaction can be expressed in terms of the derivatives of the concentrations of $N_2$,$H_2$,or $NH_3$. Write the correct relationship between the rate expressions.

Difficult

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For the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$,the rate of reaction is expressed as:

MediumAIPMT 1997

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From the concentrations of $C_{4}H_{9}Cl$ (butyl chloride) at different times given below,calculate the average rate of the reaction:
$C_{4}H_{9}Cl + H_{2}O \rightarrow C_{4}H_{9}OH + HCl$
during different intervals of time.

$t/s$ $0$ $50$ $100$ $150$ $200$ $300$ $400$ $700$ $800$

$[C_{4}H_{9}Cl]/mol\ L^{-1}$ $0.100$ $0.0905$ $0.0820$ $0.0741$ $0.0671$ $0.0549$ $0.0439$ $0.0210$ $0.017$

Difficult

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Which of the following equations is correct regarding the rate of disappearance of reactant and appearance of product for the reaction $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$?

EasyMHT CET 2025

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For the reaction, $3A + 2B \to C + D$, the differential rate law can be written as:

MediumJEE MAIN 2014

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$t/s$	$0$	$50$	$100$	$150$	$200$	$300$	$400$	$700$	$800$
$[C_{4}H_{9}Cl]/mol\ L^{-1}$	$0.100$	$0.0905$	$0.0820$	$0.0741$	$0.0671$	$0.0549$	$0.0439$	$0.0210$	$0.017$

For the reaction $2A + B \rightarrow 2C$,the rate of disappearance of $A$ is $0.076 \ mol \ s^{-1}$. What is the rate of disappearance of $B$?

Similar Questions

For the chemical reaction $N_2 + 3H_2 \rightarrow 2NH_3$,the rate of reaction can be expressed in terms of the derivatives of the concentrations of $N_2$,$H_2$,or $NH_3$. Write the correct relationship between the rate expressions.

For the reaction $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$,the rate of reaction is expressed as:

Which of the following equations is correct regarding the rate of disappearance of reactant and appearance of product for the reaction $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$?

For the reaction, $3A + 2B \to C + D$, the differential rate law can be written as:

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