For the reaction, 2N2O5→4NO2+O2, rate and rate constant are 1.02×10−4mol L−1s−1 and 3.4×10−5s−1respectively. The concentration of N2O5 at that time will be

Rate =KN2O511.02×10−4=3.4×10−5×N2O5N2O5=3M

For the reaction, 2N2O5→4NO2+O2, rate and rate constant are 1.02×10−4mol L−1s−1 and 3.4×10−5s−1respectively. The concentration of N2O5 at that time will be

Rate =KN2O511.02×10−4=3.4×10−5×N2O5N2O5=3M

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For the reaction, $2 N_{2} O_{5} \to 4 {NO}_{2} + O_{2}$ , rate and rate constant are $1 .02 \times 10^{- 4} mol L^{- 1} s^{- 1}$ and $3 .4 \times 10^{- 5} s^{- 1}$ respectively. The concentration of N₂O₅ at that time will be

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1.73 M

3 M

1.02 x 10^-4 M

3.4 x 10⁵ M

answer is B.

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$\begin{array}{l} Rate = K {[N_{2} O_{5}]}^{1} \\ 1 .02 \times 10^{- 4} = 3 .4 \times 10^{- 5} \times [N_{2} O_{5}] \\ [N_{2} O_{5}] = 3 M \end{array}$

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For the reaction, 2N2O5→4NO2+O2, rate and rate constant are 1.02×10−4mol L−1s−1 and 3.4×10−5s−1respectively. The concentration of N2O5 at that time will be

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For the reaction, $2 N_{2} O_{5} \to 4 {NO}_{2} + O_{2}$ , rate and rate constant are $1 .02 \times 10^{- 4} mol L^{- 1} s^{- 1}$ and $3 .4 \times 10^{- 5} s^{- 1}$ respectively. The concentration of N₂O₅ at that time will be