(D) For the reaction,$N_2 + 3H_2 \rightarrow 2NH_3,$ the rate of reaction is given by:Rate $= -\frac{d[N_2]}{dt} = -\frac{1}{3} \frac{d[H_2]}{dt} = \f

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(D) For the reaction,$N_2 + 3H_2 \rightarrow 2NH_3,$ the rate of reaction is given by:Rate $= -\frac{d[N_2]}{dt} = -\frac{1}{3} \frac{d[H_2]}{dt} = \frac{1}{2} \frac{d[NH_3]}{dt}$Given that $\frac{d[NH_3]}{dt} = 2 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}.$Equating the terms for $H_2$ and $NH_3$:$-\frac{1}{3} \frac{d[H_2]}{dt} = \frac{1}{2} \frac{d[NH_3]}{dt}$$-\frac{d[H_2]}{dt} = \frac{3}{2} \times \frac{d[NH_3]}{dt}$$-\frac{d[H_2]}{dt} = \frac{3}{2} \times (2 \times 10^{-4}) = 3 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}.$

Class 12 Chemistry Chemical Kinetics Rate of a reaction

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For the reaction,$N_2 + 3H_2 \rightarrow 2NH_3,$ if $\frac{d[NH_3]}{dt} = 2 \times 10^{-4} \ mol \ L^{-1} \ s^{-1},$ the value of $-\frac{d[H_2]}{dt}$ would be .................. $mol \ L^{-1} \ s^{-1}$.

AIPMT 2009 All AIPMT

A
$4 \times 10^{-4}$
B
$6 \times 10^{-4}$
C
$1 \times 10^{-4}$
D
$3 \times 10^{-4}$

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In the reaction $2SO_3 \to 2SO_2 + O_2$,initially $40 \ g$ of $SO_3$ is heated in a $100 \ mL$ container. If after $10 \ min$,$3.2 \ g$ of $O_2$ is formed,find the rate of reaction in $mol \ L^{-1} \ min^{-1}$.

Medium

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Why is the rate of reaction expressed as negative with respect to a reactant? Is the rate of reaction really negative?

Easy

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For the reaction,$3 I_{(aq)}^{-} + S_2 O_{8_{(aq)}}^{2-} \longrightarrow 2 SO_{4_{(aq)}}^{2-} + I_{3_{(aq)}}^{-}$,the rate of formation of $SO_{4_{(aq)}}^{2-}$ is $0.044 \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate of consumption of $I_{(aq)}^{-}$.

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$A \rightarrow P$ is a first-order reaction. The following graph is obtained for this reaction ($x$-axis $=$ time,$y$-axis $=$ concentration of $A$). The instantaneous rate of the reaction at point $C$ is:

MediumAP EAMCET 2021

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Assertion : The rate of the reaction is the rate of change of concentration of a reactant or a product.
Reason : Rate of reaction remains constant during the course of reaction.

MediumAIIMS 2010

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For the reaction,$N_2 + 3H_2 \rightarrow 2NH_3,$ if $\frac{d[NH_3]}{dt} = 2 \times 10^{-4} \ mol \ L^{-1} \ s^{-1},$ the value of $-\frac{d[H_2]}{dt}$ would be .................. $mol \ L^{-1} \ s^{-1}$.

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In the reaction $2SO_3 \to 2SO_2 + O_2$,initially $40 \ g$ of $SO_3$ is heated in a $100 \ mL$ container. If after $10 \ min$,$3.2 \ g$ of $O_2$ is formed,find the rate of reaction in $mol \ L^{-1} \ min^{-1}$.

Why is the rate of reaction expressed as negative with respect to a reactant? Is the rate of reaction really negative?

For the reaction,$3 I_{(aq)}^{-} + S_2 O_{8_{(aq)}}^{2-} \longrightarrow 2 SO_{4_{(aq)}}^{2-} + I_{3_{(aq)}}^{-}$,the rate of formation of $SO_{4_{(aq)}}^{2-}$ is $0.044 \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate of consumption of $I_{(aq)}^{-}$.

$A \rightarrow P$ is a first-order reaction. The following graph is obtained for this reaction ($x$-axis $=$ time,$y$-axis $=$ concentration of $A$). The instantaneous rate of the reaction at point $C$ is:

Assertion : The rate of the reaction is the rate of change of concentration of a reactant or a product.Reason : Rate of reaction remains constant during the course of reaction.

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Assertion : The rate of the reaction is the rate of change of concentration of a reactant or a product.
Reason : Rate of reaction remains constant during the course of reaction.