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Chemistry Question on Chemical Kinetics

For the chemical reaction N2(g)+3H2(g)⇌2NH3(g)N_{2 (g)} +3H_{2(g)} \rightleftharpoons 2NH_{3(g)} the correct option is :

A

−d[N2]dt=12d[NH3]dt-\frac{d\left[N_{2}\right]}{dt}=\frac{1}{2}\frac{d\left[NH_{3}\right]}{dt}

B

3d[H2]dt=2d[NH3]dt3\frac{d\left[H_{2}\right]}{dt}=2\frac{d\left[NH_{3}\right]}{dt}

C

−13d[H2]dt=2d[NH3]dt-\frac{1}{3}\frac{d\left[H_{2}\right]}{dt}=2\frac{d\left[NH_{3}\right]}{dt}

D

−d[N2]dt=2d[NH3]dt-\frac{d\left[N_{2}\right]}{dt}=2\frac{d\left[NH_{3}\right]}{dt}

Answer

−d[N2]dt=12d[NH3]dt-\frac{d\left[N_{2}\right]}{dt}=\frac{1}{2}\frac{d\left[NH_{3}\right]}{dt}

Explanation

Solution

N2+3H2<=>2NH3{N_2 + 3H_2 <=> 2NH_3}
Rate of reaction is given as
−d[N2]dt=−13d[H2]dt=+12d[NH3]dt- \frac{d\left[N_{2}\right]}{dt} = - \frac{1}{3} \frac{d\left[H_{2}\right]}{dt} =+ \frac{1}{2} \frac{d\left[NH_{3}\right]}{dt}