For the reaction $2N_2O_{5(g)} \to 4NO_{2(g)} + O_{2(g)}$,if the concentration of $NO_2$ increases by $5.2 \times 10^{-3} \ M$ in $100 \ s$,then the rate of reaction will be:
- A$1.3 \times 10^{-5} \ M \ s^{-1}$
- B$5 \times 10^{-4} \ M \ s^{-1}$
- C$7.6 \times 10^{-4} \ M \ s^{-1}$
- D$2 \times 10^{-3} \ M \ s^{-1}$
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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:
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