For the reaction $3A \to 2B$,the rate of reaction is expressed as $\frac{+d[B]}{dt} = \dots$

For the reaction $2N_2O_{5(g)} \rightleftharpoons 4NO_{2(g)} + O_{2(g)}$ in a closed vessel,the concentration of $NO_2$ increases by $2.0 \times 10^{-2} \, mol \, L^{-1}$ in $5 \, s$. Calculate the rate of reaction.

Explain: What is instantaneous rate? How is it determined?

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.

Consider the elementary reaction $A_{(g)} + B_{(g)} \rightarrow C_{(g)} + D_{(g)}$. If the volume of the reaction mixture is suddenly reduced to $\frac{1}{3}$ of its initial volume,the reaction rate will become '$x$' times the original reaction rate. The value of $x$ is:

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: