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Question: The reaction \(N_{2}O_{5}(\text{in}CCl_{4}\text{solution}) \rightarrow 2NO_{2}(\text{solution}) + \...

The reaction

N2O5(inCCl4solution)→2NO2(solution)+12O2(g)N_{2}O_{5}(\text{in}CCl_{4}\text{solution}) \rightarrow 2NO_{2}(\text{solution}) + \frac{1}{2}O_{2}(g)

is of first order in N2O5N_{2}O_{5} with rate constant 6.2×10−1s−1.6.2 \times 10^{- 1}s^{- 1}.

What is the value of rate of reaction when

[N2O5]=1.25molel−1\lbrack N_{2}O_{5}\rbrack = 1.25molel^{- 1}.

A

7.75×10−1molel−1s−17.75 \times 10^{- 1}molel^{- 1}s^{- 1}

B

6.35×10−3molel−1s−16.35 \times 10^{- 3}molel^{- 1}s^{- 1}

C

5.15×10−5molel−1s−15.15 \times 10^{- 5}molel^{- 1}s^{- 1}

D

3.85×10−1molel−1s−13.85 \times 10^{- 1}molel^{- 1}s^{- 1}

Answer

7.75×10−1molel−1s−17.75 \times 10^{- 1}molel^{- 1}s^{- 1}

Explanation

Solution

Rate =K(N2O5)=6.2×10−1×1.25= K(N_{2}O_{5}) = 6.2 \times 10^{- 1} \times 1.25

=7.75×10−1moll−1s−1= 7.75 \times 10^{- 1}moll^{- 1}s^{- 1}