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

For the reaction 2N2O5→4NO2+O22N_{2}O_{5} \rightarrow 4NO_{2} + O_{2}rate of reaction and rate constant are 1.02×10−41.02 \times 10^{- 4}and 3.4×10−5sec⁡−13.4 \times 10^{- 5}\sec^{- 1}{}

respectively. The concentration of N2O5N_{2}O_{5} at that time will be.

A

1.7321.732

B

3

C

1.02×10−41.02 \times 10^{- 4}

D

3.4×1053.4 \times 10^{5}

Answer

3

Explanation

Solution

R=K[A]R = K\lbrack A\rbrack, 1.02×10−4=3.4×10−5,[N2O5]1.02 \times 10^{- 4} = 3.4 \times 10^{- 5},\lbrack N_{2}O_{5}\rbrack

or (N2O5)=1.02×10−43.4×10−5,K=3(N_{2}O_{5}) = \frac{1.02 \times 10^{- 4}}{3.4 \times 10^{- 5}},K = 3