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 $NO_2$?
- A$4 \times 10^{-3} \ M \ s^{-1}$
- B$10^{-3} \ M \ s^{-1}$
- C$2 \times 10^{-3} \ M \ s^{-1}$
- D$10^{-2} \ M \ s^{-1}$
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View SolutionConsider a gas phase reaction which occurs in a closed vessel: $2 \ A \rightarrow 4 \ B + C$. The concentration of $B$ is found to be increased by $5 \times 10^{-3} \ mol \ L^{-1}$ in $10 \ s$. The rate of disappearance of $A$ (in $mol \ L^{-1} \ s^{-1}$) is:
For the reaction $2P + Q \to R$. If the rate of appearance of $R$ is $0.5 \ mol \ L^{-1} \ h^{-1}$,then the rate of disappearance of $P$ and $Q$ are:
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