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Question: For the reaction \(2N_{2}O_{5}\overset{\quad\quad}{\rightarrow}4NO_{2} + O_{2},\) the rate of reacti...

For the reaction 2N2O5→4NO2+O2,2N_{2}O_{5}\overset{\quad\quad}{\rightarrow}4NO_{2} + O_{2}, the rate of reaction can be expressed in terms of time and concentration by the expression:

A

Rate=d[N2O5]dt=−14d[NO2]dt=12d[O2]dtRate = \frac{d\lbrack N_{2}O_{5}\rbrack}{dt} = - \frac{1}{4}\frac{d\lbrack NO_{2}\rbrack}{dt} = \frac{1}{2}\frac{d\lbrack O_{2}\rbrack}{dt}

B

Rate=−12d[N2O5]dt=14d[NO2]dt=d[O2]dtRate = - \frac{1}{2}\frac{d\lbrack N_{2}O_{5}\rbrack}{dt} = \frac{1}{4}\frac{d\lbrack NO_{2}\rbrack}{dt} = \frac{d\lbrack O_{2}\rbrack}{dt}

C

Rate=−14d[N2O5]dt=12d[NO2]dt=d[O2]dtRate = - \frac{1}{4}\frac{d\lbrack N_{2}O_{5}\rbrack}{dt} = \frac{1}{2}\frac{d\lbrack NO_{2}\rbrack}{dt} = \frac{d\lbrack O_{2}\rbrack}{dt}

D

Rate=−12d[N2O5]dt=12d[NO2]dt=12d[O2]dtRate = - \frac{1}{2}\frac{d\lbrack N_{2}O_{5}\rbrack}{dt} = \frac{1}{2}\frac{d\lbrack NO_{2}\rbrack}{dt} = \frac{1}{2}\frac{d\lbrack O_{2}\rbrack}{dt}

Answer

Rate=−12d[N2O5]dt=14d[NO2]dt=d[O2]dtRate = - \frac{1}{2}\frac{d\lbrack N_{2}O_{5}\rbrack}{dt} = \frac{1}{4}\frac{d\lbrack NO_{2}\rbrack}{dt} = \frac{d\lbrack O_{2}\rbrack}{dt}

Explanation

Solution

For 2N2O5→4NO2+O22N_{2}O_{5} \rightarrow 4NO_{2} + O_{2} the rate of reaction can be expressed as

−12d[N2O5]dt=14d[NO2]dt=d[O2]dt- \frac{1}{2}\frac{d\lbrack N_{2}O_{5}\rbrack}{dt} = \frac{1}{4}\frac{d\lbrack NO_{2}\rbrack}{dt} = \frac{d\lbrack O_{2}\rbrack}{dt}