(A) For the reaction $2SO_{2(g)} + O_{2(g)} \rightarrow 2SO_{3(g)}$,the rate of reaction is expressed as:$Rate = -\frac{1}{2} \frac{d[SO_2]}{dt} = -\f

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(A) For the reaction $2SO_{2(g)} + O_{2(g)} \rightarrow 2SO_{3(g)}$,the rate of reaction is expressed as:$Rate = -\frac{1}{2} \frac{d[SO_2]}{dt} = -\frac{d[O_2]}{dt} = \frac{1}{2} \frac{d[SO_3]}{dt}$Given that $-\frac{d[O_2]}{dt} = 2.5 \times 10^{-4} \, mol \, L^{-1} \, s^{-1}$.Equating the terms for $SO_2$ and $O_2$:$-\frac{1}{2} \frac{d[SO_2]}{dt} = -\frac{d[O_2]}{dt}$$-\frac{d[SO_2]}{dt} = 2 \times (-\frac{d[O_2]}{dt})$$-\frac{d[SO_2]}{dt} = 2 \times (2.5 \times 10^{-4} \, mol \, L^{-1} \, s^{-1}) = 5 \times 10^{-4} \, mol \, L^{-1} \, s^{-1}$.

Class 12 Chemistry Chemical Kinetics Rate of a reaction

Medium

In the contact process for the manufacture of sulfur trioxide,the reaction is $2SO_{2(g)} + O_{2(g)} \rightarrow 2SO_{3(g)}$. If the rate of reaction is given by $-\frac{d[O_2]}{dt} = 2.5 \times 10^{-4} \, mol \, L^{-1} \, s^{-1}$,what is the rate of disappearance of $SO_2$?

A
$5 \times 10^{-4} \, mol \, L^{-1} \, s^{-1}$
B
$2.5 \times 10^{-4} \, mol \, L^{-1} \, s^{-1}$
C
$1.25 \times 10^{-4} \, mol \, L^{-1} \, s^{-1}$
D
$7.5 \times 10^{-4} \, mol \, L^{-1} \, s^{-1}$

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Class 12

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Chemical Kinetics

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Rate of a reaction

The velocity of disappearance for $HI$ is $2.4 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$. Calculate the rate of formation of $H_2$.

Medium

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Consider the reaction, $3I^-_{(aq)} + S_2O_8^{2-} (aq) \rightarrow I_3^- (aq) + 2SO_4^{2-} (aq)$. If the rate of formation of $SO_4^{2-}$ at a particular time is $2.2 \times 10^{-2} \text{ mol dm}^{-3} \text{s}^{-1}$, calculate the rate of consumption of $I^-$.

DifficultMHT CET 2026

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

Medium

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For the chemical reaction: $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$,the rate of reaction can be expressed in terms of the concentration of $N_{2(g)}$,$H_{2(g)}$,or $NH_{3(g)}$ with respect to time. Identify the correct relationship between these rates.

Medium

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In the contact process for the manufacture of sulfur trioxide,the reaction is $2SO_{2(g)} + O_{2(g)} \rightarrow 2SO_{3(g)}$. If the rate of reaction is given by $-\frac{d[O_2]}{dt} = 2.5 \times 10^{-4} \, mol \, L^{-1} \, s^{-1}$,what is the rate of disappearance of $SO_2$?

Similar Questions

The velocity of disappearance for $HI$ is $2.4 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$. Calculate the rate of formation of $H_2$.

Consider the reaction, $3I^-_{(aq)} + S_2O_8^{2-} (aq) \rightarrow I_3^- (aq) + 2SO_4^{2-} (aq)$. If the rate of formation of $SO_4^{2-}$ at a particular time is $2.2 \times 10^{-2} \text{ mol dm}^{-3} \text{s}^{-1}$, calculate the rate of consumption of $I^-$.

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?

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

For the chemical reaction: $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$,the rate of reaction can be expressed in terms of the concentration of $N_{2(g)}$,$H_{2(g)}$,or $NH_{3(g)}$ with respect to time. Identify the correct relationship between these rates.

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