(D) For the reaction $2SO_2 + O_2 \rightleftharpoons 2SO_3$,the rate of reaction is expressed as:Rate $= -\frac{1}{2} \frac{d[SO_2]}{dt} = -\frac{d[O_

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(D) For the reaction $2SO_2 + O_2 \rightleftharpoons 2SO_3$,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})$$\frac{d[SO_2]}{dt} = -5.00 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$.

Class 12 Chemistry Chemical Kinetics Rate of a reaction

Difficult

In the reaction of formation of sulphur trioxide by contact process $2SO_2 + O_2 \rightleftharpoons 2SO_3$,the rate of reaction was measured as $\frac{d[O_2]}{dt} = -2.5 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$. The rate of reaction in terms of $[SO_2]$ in $mol \ L^{-1} \ s^{-1}$ will be:

JEE MAIN 2014 All JEE MAIN

A
$-1.25 \times 10^{-4}$
B
$-2.50 \times 10^{-4}$
C
$-3.75 \times 10^{-4}$
D
$-5.00 \times 10^{-4}$

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Chemical Kinetics

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Rate of a reaction

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Consider the graph given in the following diagram. Which of the following options does not show the instantaneous rate of reaction at the $40^{th}$ second?

Medium

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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 $I_{(aq)}^{-}$.

DifficultMHT CET 2024

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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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For the reaction $5Br_{(aq)}^{-} + BrO_{3_{(aq)}}^{-} + 6H_{(aq)}^{+} \rightarrow 3Br_{2_{(aq)}} + 3H_{2}O_{(l)}$,if $\frac{-\Delta[Br^{-}]}{\Delta t} = 4.2 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$,calculate the rate of formation of $Br_{2}$,i.e.,$\frac{\Delta[Br_{2}]}{\Delta t}$.

Medium

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For the reaction $2A + B \rightarrow 3C + D$,which of the following options does not represent the correct rate of the reaction?

Medium

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In the reaction of formation of sulphur trioxide by contact process $2SO_2 + O_2 \rightleftharpoons 2SO_3$,the rate of reaction was measured as $\frac{d[O_2]}{dt} = -2.5 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$. The rate of reaction in terms of $[SO_2]$ in $mol \ L^{-1} \ s^{-1}$ will be:

Similar Questions

Consider the graph given in the following diagram. Which of the following options does not show the instantaneous rate of reaction at the $40^{th}$ second?

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 $I_{(aq)}^{-}$.

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 $I^-$.

For the reaction $5Br_{(aq)}^{-} + BrO_{3_{(aq)}}^{-} + 6H_{(aq)}^{+} \rightarrow 3Br_{2_{(aq)}} + 3H_{2}O_{(l)}$,if $\frac{-\Delta[Br^{-}]}{\Delta t} = 4.2 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$,calculate the rate of formation of $Br_{2}$,i.e.,$\frac{\Delta[Br_{2}]}{\Delta t}$.

For the reaction $2A + B \rightarrow 3C + D$,which of the following options does not represent the correct rate of the reaction?

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