question_answer

Consider the chemical reaction: \[{{N}_{2}}(g)+3{{H}_{2}}(g)\xrightarrow{{}}2N{{H}_{3}}(g)\] The rate of this reaction can be expressed in terms of time derivative of concentration of \[{{N}_{2}}(g),{{H}_{2}}(g)\]or\[N{{H}_{3}}(g)\]. Identify the correct relationship amongst the rate expressions:

A)  \[rate=-\frac{d[{{N}_{2}}]}{dt}=-\frac{1}{3}\frac{d[{{H}_{2}}]}{dt}=\frac{1}{2}\frac{d[N{{H}_{3}}]}{dt}\]

B)  \[rate=-\frac{d[{{N}_{2}}]}{dt}=-3\frac{d[{{H}_{2}}]}{dt}=2\frac{d[N{{H}_{3}}]}{dt}\]

C)  \[rate=\frac{d[{{N}_{2}}]}{dt}=\frac{1}{3}\frac{d[{{H}_{2}}]}{dt}=\frac{1}{2}\frac{d[N{{H}_{3}}]}{dt}\]

D)  \[rate=-\frac{d[{{N}_{2}}]}{dt}=-\frac{d[{{H}_{2}}]}{dt}=\frac{d[N{{H}_{3}}]}{dt}\]