1. -1/3d[H₂]/dt = -1/2d[NH₃]/dt 2. -d[N₂]/dt = 2d[NH₃]/dt 3. -d[N₂]/dt = 1/2d[NH₃]/dt 4. 3d[H₂]/dt = 2d[NH₃]/dt

Answer: 3. -d[N₂]/dt = 1/2d[NH₃]/dt Rate of reaction: divide the rate of change of each species by its stoichiometric coefficient (negative for reactants). rate = -d[N₂]/dt = -1/3d[H₂]/dt = 1/2d[NH₃]/dt So -d[N₂]/dt = 1/2d[NH₃]/dt , option (3). Option (1) has a wrong sign, (2) wrong factor, (4) wrong sign and factor.

Topic: Rate of reaction and factors affecting it· Chemical Kinetics

For the chemical reactionN_2(g) + 3H_2(g) ⇌ 2NH_3(g)the correct option is :

1. \(-\frac{1}{3}\frac{d[H_2]}{dt} = -\frac{1}{2}\frac{d[NH_3]}{dt}\)

2. \(-\frac{d[N_2]}{dt} = 2\frac{d[NH_3]}{dt}\)

3. \(-\frac{d[N_2]}{dt} = \frac{1}{2}\frac{d[NH_3]}{dt}\)

4. \(3\frac{d[H_2]}{dt} = 2\frac{d[NH_3]}{dt}\)

Doubtly Asked 30 Oct 2026 NEET UG 2019 Practice test neet Save WhatsApp Report

1 answer

Best answer

Answer: 3. \(-\frac{d[N_2]}{dt} = \frac{1}{2}\frac{d[NH_3]}{dt}\)

Rate of reaction: divide the rate of change of each species by its stoichiometric coefficient (negative for reactants).

\(\text{rate} = -\dfrac{d[N_2]}{dt} = -\dfrac{1}{3}\dfrac{d[H_2]}{dt} = \dfrac{1}{2}\dfrac{d[NH_3]}{dt}\)

So \(-\dfrac{d[N_2]}{dt} = \dfrac12\dfrac{d[NH_3]}{dt}\), option (3). Option (1) has a wrong sign, (2) wrong factor, (4) wrong sign and factor.

Doubtly AI · 30 Oct 2026 AI-generated · not yet verified Report

Was this answer helpful?

For the chemical reactionN_2(g) + 3H_2(g) ⇌ 2NH_3(g)the correct option is :

1 answer

Your answer