(C) For the reaction $2A + B \to A_2B$,the rate of reaction is given by: $Rate = -\frac{1}{2} \frac{d[A]}{dt} = -\frac{d[B]}{dt} = \frac{d[A_2B]}{dt}$

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Twice the rate that $B$ will decrease

(C) For the reaction $2A + B \to A_2B$,the rate of reaction is given by: $Rate = -\frac{1}{2} \frac{d[A]}{dt} = -\frac{d[B]}{dt} = \frac{d[A_2B]}{dt}$ From the expression $-\frac{1}{2} \frac{d[A]}{dt} = -\frac{d[B]}{dt}$,we get: $-\frac{d[A]}{dt} = 2 \times (-\frac{d[B]}{dt})$ This shows that the rate of disappearance of $A$ $(-\frac{d[A]}{dt})$ is twice the rate of disappearance of $B$ $(-\frac{d[B]}{dt})$.

Class 12 Chemistry Chemical Kinetics Rate of a reaction

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In a reaction $2A + B \to A_2B$,the reactant $A$ will disappear at

A
Half the rate that $B$ will decrease
B
The same rate that $B$ will decrease
C
Twice the rate that $B$ will decrease
D
The same rate that $A_2B$ will form

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Rate of a reaction

Consider the following reaction: $2 NO_{2(g)} + F_{2(g)} \longrightarrow 2 NO_2F_{(g)}$. The expression for the rate of reaction in terms of the rate of change of partial pressure of reactant and product is/are:

MediumWBJEE 2013

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Observe the following reaction: $2 A + B \longrightarrow C$. The rate of formation of $C$ is $2.2 \times 10^{-3} \ mol \ L^{-1} \ min^{-1}$. What is the value of $-\frac{d[A]}{d t}$ (in $mol \ L^{-1} \ min^{-1}$)?

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For the reaction $4KClO_3 \to 3KClO_4 + KCl$,if $-d[KClO_3]/dt = K_1[KClO_3]^4$,$d[KClO_4]/dt = K_2[KClO_3]^4$,and $d[KCl]/dt = K_3[KClO_3]^4$,then:

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Write the rate equation for the following reactions:
$1.$ $2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$
$2.$ $2 HI_{(g)} \rightarrow H_{2(g)} + I_{2(g)}$

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If the first order reaction involves gaseous reactants and gaseous products,the units of its rate are:

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In a reaction $2A + B \to A_2B$,the reactant $A$ will disappear at

Similar Questions

Consider the following reaction: $2 NO_{2(g)} + F_{2(g)} \longrightarrow 2 NO_2F_{(g)}$. The expression for the rate of reaction in terms of the rate of change of partial pressure of reactant and product is/are:

Observe the following reaction: $2 A + B \longrightarrow C$. The rate of formation of $C$ is $2.2 \times 10^{-3} \ mol \ L^{-1} \ min^{-1}$. What is the value of $-\frac{d[A]}{d t}$ (in $mol \ L^{-1} \ min^{-1}$)?

For the reaction $4KClO_3 \to 3KClO_4 + KCl$,if $-d[KClO_3]/dt = K_1[KClO_3]^4$,$d[KClO_4]/dt = K_2[KClO_3]^4$,and $d[KCl]/dt = K_3[KClO_3]^4$,then:

Write the rate equation for the following reactions:$1.$ $2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$$2.$ $2 HI_{(g)} \rightarrow H_{2(g)} + I_{2(g)}$

If the first order reaction involves gaseous reactants and gaseous products,the units of its rate are:

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Write the rate equation for the following reactions:
$1.$ $2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$
$2.$ $2 HI_{(g)} \rightarrow H_{2(g)} + I_{2(g)}$