A) \[\frac{1}{2}\frac{d}{dt}[{{N}_{2}}{{O}_{5}}]\]
B) \[2\frac{d}{dt}[{{N}_{2}}{{O}_{5}}]\]
C) \[\frac{1}{4}\frac{d}{dt}[N{{O}_{2}}]\]
D) \[4\frac{d}{dt}[N{{O}_{2}}]\]
Correct Answer: C
Solution :
\[2{{N}_{2}}{{O}_{5}}\xrightarrow{{}}4N{{O}_{2}}+{{O}_{2}}\] rate of reaction is: \[\frac{1}{2}\frac{d[{{N}_{2}}{{O}_{5}}]}{dt}=\frac{1}{4}\frac{d[N{{O}_{2}}]}{dt}\] So, rate of disappearance of \[{{N}_{2}}{{O}_{5}}\] is represented either by \[-\frac{1}{2}\frac{[{{N}_{2}}{{O}_{5}}]}{dt}\] or by \[\frac{1}{4}\frac{d[N{{O}_{2}}]}{dt}\]
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