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Chemistry Question on Chemical Kinetics

For the reaction, 2N2O5→4NO2+O22N_{2}O_{5} \to 4NO_{2} + O_{2} rate and rate constant are 1.02×10−4 mol L−1s−11.02 \times 10^{-4}\,mol\, L^{-1} s^{-1} and 3.4×10−5s−13.4 \times 10^{-5} s^{-1} respectively. The concentration of N2O5N_{2}O_{5} in mol L−1L^{-1} will be

A

3.4×10−43.4 \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

The correct answer is B:3.0
[N2O5]=Ratek=1.02×10−4mol L−1 s−13.4×10−5s−1\left[N_{2}O_{5}\right]=\frac{Rate}{k}=\frac{1.02\times10^{-4}mol \,L^{-1}\,s^{-1}}{3.4\times10^{-5} s^{-1}}
=3 mol L−1=3\,mol\,L^{-1}