For the reaction $2N_2O_5 \rightarrow 4NO_2 + O_2$,if the concentration of $NO_2$ increases by $1.6 \times 10^{-2} \ M$ in $4 \ seconds$,what is the rate of formation of $NO_2$?

The concentration of a reactant changes from $0.1 \, mol \, L^{-1}$ to $0.095 \, mol \, L^{-1}$ in $10 \, s$. Calculate the rate of reaction.

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:

The average rate of reaction $2SO_{2(g)} + O_{2(g)} \rightarrow 2SO_{3(g)}$ is written as

In a reaction,$2 A \rightarrow \text{Products}$,the concentration of $A$ decreases from $0.5 \ mol \ L^{-1}$ to $0.4 \ mol \ L^{-1}$ in $10 \ minutes$. Calculate the rate during this interval?

For the reaction $3 A + 2 B \rightarrow C$,which statement is correct $:-$