The instantaneous rate of a reaction is given by $-\frac{1}{2} \frac{d[x]}{dt} = -\frac{d[y]}{dt} = \frac{1}{2} \frac{d[z]}{dt}$. Identify the reaction.
- A$2x + y \longrightarrow 2z$
- B$x + 2y \longrightarrow 2z$
- C$2z + y \longrightarrow 2x$
- D$2x + 2y \longrightarrow z$
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For the reaction,$A + 3B \longrightarrow 2C$,the rate of consumption of $A$ is $1.4 \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate of formation of $C$.
What is the rate of formation of $O_2$ for the reaction stated below?
$2 N_2O_{5(g)} \longrightarrow 4 NO_{2(g)} + O_{2(g)}$
Given: $\left| \frac{d[N_2O_5]}{dt} \right| = 0.02 \ mol \ dm^{-3} \ s^{-1}$
$2 N_2O_{5(g)} \longrightarrow 4 NO_{2(g)} + O_{2(g)}$
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In the reaction,$BrO_{3(aq)}^{-} + 5Br_{(aq)}^{-} + 6H^{+} \to 3Br_{2(l)} + 3H_2O_{(l)}$. The rate of appearance of bromine $(Br_2)$ is related to the rate of disappearance of bromide ions as:
MediumAIPMT 2009
View SolutionExplain the relation between the rate of reaction and the stoichiometric coefficients of a balanced chemical equation with examples.
Difficult
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