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Question: Consider the reaction \(2N_{2}O_{5}\overset{\quad\quad}{\rightarrow}4NO_{2} + O_{2}.\) In the react...

Consider the reaction 2N2O54NO2+O2.2N_{2}O_{5}\overset{\quad\quad}{\rightarrow}4NO_{2} + O_{2}.

In the reaction NO2NO_{2} is being formed at the rate of 0.0125molL0.0125molL. What is rate of reaction at this time?

A

0.0018molL1s10.0018molL^{- 1}s^{- 1}

B

0.0031molL1s10.0031molL^{- 1}s^{- 1}

C

0.0041molL1s10.0041molL^{- 1}s^{- 1}

D

0.050molL1s10.050molL^{- 1}s^{- 1}

Answer

0.0031molL1s10.0031molL^{- 1}s^{- 1}

Explanation

Solution

Rate=14d[NO2]dt=14×0.0125=0.0031molL1s1Rate = \frac{1}{4}\frac{d\lbrack NO_{2}\rbrack}{dt} = \frac{1}{4} \times 0.0125 = 0.0031molL^{- 1}s^{- 1}