For the reaction $\frac{1}{2} A \rightarrow 2B$,the rate of disappearance of $A$ is related to the rate of appearance of $B$ by which of the following expressions?
- A$-\frac{d[A]}{dt} = \frac{1}{2} \frac{d[B]}{dt}$
- B$-\frac{d[A]}{dt} = \frac{1}{4} \frac{d[B]}{dt}$
- C$-\frac{d[A]}{dt} = \frac{d[B]}{dt}$
- D$-\frac{d[A]}{dt} = 4 \frac{d[B]}{dt}$
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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 $I^-$.
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View SolutionFind the average rate of formation of $NO_{2_{(g)}}$ in the following reaction:
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For a general chemical reaction $2A + 3B \rightarrow \text{Products}$,if the rate of disappearance of $A$ is $r_1$ and that of $B$ is $r_2$,then the relationship between $r_1$ and $r_2$ is:
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View SolutionFor the reaction,$2N_2O_{5(g)} \rightarrow 4NO_{2(g)} + O_{2(g)}$,the rate of formation of $O_2$ is $0.032 \ g \ h^{-1}$. What is the rate of conversion of $N_2O_5$ in $g \ h^{-1}$?
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