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Question: For the reaction \(2N_{2}O_{5} \rightarrow 4NO_{2} + O_{2}\) rate and rate constant are \(1.02 \time...

For the reaction 2N2O5→4NO2+O22N_{2}O_{5} \rightarrow 4NO_{2} + O_{2} rate and rate constant are 1.02×10−4molL−1s−11.02 \times 10^{- 4}molL^{- 1}s^{- 1} and 3.4×10−5s−13.4 \times 10^{- 5}s^{- 1} respectively. The concentration of N2ON_{2}Oin molL−1molL^{- 1} will be

A

3.4×1043.4 \times 10^{4}

B

3.03.0

C

5.25.2

D

3.2×10−53.2 \times 10^{- 5}

Answer

3.03.0

Explanation

Solution

[N2O2]=Ratek=1.02×10−4molL−1s−13.4×10−5s−1=3molL−1\lbrack N_{2}O_{2}\rbrack = \frac{Rate}{k} = \frac{1.02 \times 10^{- 4}molL^{- 1}s^{- 1}}{3.4 \times 10^{- 5}s^{- 1}} = 3molL^{- 1}