For the given elementary reaction N 2 + 3 H 2 → 2 N H 3 if Δ [ N H 3 ] Δ t = 2 × 1 0 - 4 m o l L - 1 s - 1 , then calculate value of - Δ [ H 2 ] Δ t

N 2 + 3 H 2 ⇌ 2 N H 3 - Δ [ N 2 ] Δ t = - 1 3 Δ [ H 2 ] Δ t = 1 2 Δ [ N H 3 ] Δ t ∴ Δ [ H 2 ] Δ t = 3 2 × Δ [ N H 3 ] Δ t = 3 2 × 2 × 1 0 - 4 = 3 × 10 − 4 molL − 1 s − 1

Chemistry - Chemical Kinetics Question with Solution | TestHub

ChemistryChemical KineticsRate of Reactions/Rate LawEasy2 minPYQ_2020

ChemistryEasysingle choice

For the given elementary reaction $N_{2} + 3 H_{2} \to 2 N H_{3}$ if $\frac{Δ [N H_{3}]}{Δ t} = 2 \times 1 0^{- 4} m o l L^{- 1} s^{- 1},$ then calculate value of $\frac{- Δ [H_{2}]}{Δ t}$

Options:

Answer:

Solution:

$N_{2} + 3 H_{2} ⇌ 2 N H_{3}$
$\frac{- Δ [N_{2}]}{Δ t} = - \frac{1}{3} \frac{Δ [H_{2}]}{Δ t} = \frac{1}{2} \frac{Δ [N H_{3}]}{Δ t}$
$∴ \frac{Δ [H_{2}]}{Δ t} = \frac{3}{2} \times \frac{Δ [N H_{3}]}{Δ t} = \frac{3}{2} \times 2 \times 1 0^{- 4}$
$= 3 \times 10^{- 4} {molL}^{- 1} s^{- 1}$

Stream:NTA_ABHYAS_NEETSubject:ChemistryTopic:Chemical KineticsSubtopic:Rate of Reactions/Rate Law

⏱ 2mℹ️ Source: PYQ_2020

Doubts & Discussion

Loading discussions...