Solveeit Logo
Login

Question

Question: The rate constant for the reaction \(2N_{2}O_{5} \rightarrow 4NO_{2} + O_{2}\) is \(2 \times 10^{- 5...

The rate constant for the reaction 2N2O5→4NO2+O22N_{2}O_{5} \rightarrow 4NO_{2} + O_{2} is 2×10−5s−1.2 \times 10^{- 5}s^{- 1}. If rate of reaction is 1.4×10−5molL−1s−11.4 \times 10^{- 5}molL^{- 1}s^{- 1} what will be the concentration of N2O5N_{2}O_{5} in mol L−1?L^{- 1}?

A

0.80.8

B

0.70.7

C

1.21.2

D

1

Answer

0.70.7

Explanation

Solution

Rate =k[N2O5]= k\lbrack N_{2}O_{5}\rbrack (first order as unit of rate constant iss−1s^{- 1})

[N2O5]=ratek=1.4×10−5molL−1s−12×10−5s−1=0.7molL−1\lbrack N_{2}O_{5}\rbrack = \frac{rate}{k} = \frac{1.4 \times 10^{- 5}molL^{- 1}s^{- 1}}{2 \times 10^{- 5}s^{- 1}} = 0.7molL^{- 1}