Consider the chemical reaction, N 2 ( g ) + 3 H 2 ( g ) → 2 NH 3 ( g ) The rate of reaction may be expressed as:

N 2 ( g ) + 3 H 2 ( g ) → 2 NH 3 ( g ) − dt d [ N 2 ] = − 3 1 dt d [ H 2 ] = + 2 1 dt d [ NH 3 ] = Rate of reaction.

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ChemistryChemical KineticsRate of Reactions/Rate LawMedium2 minQB

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Passage / Comprehension

The reaction rate is the increase in molar concentration of product of a reaction per unit time or the decrease in molar concentration of reactant per unit time. However, due to the stoichiometry of the balanced chemical reaction, rates of reactions in terms of individual reactants and products are related.

$m_{1} A + m_{2} B \to n_{1} C + n_{2} D$ ,

Instantaneous rate of reaction = $- \frac{1}{m _{1}} \frac{d [ A ]}{d t} = - \frac{1}{m _{2}} \frac{d [ B ]}{d t} = + \frac{1}{n _{1}} \frac{d [ C ]}{d t} = + \frac{1}{n _{2}} \frac{d [ D ]}{d t}$

In appreciable interval of time, the average rate of reaction may be given as:

Average rate of reaction = $- \frac{1}{m _{1}} \frac{Δ [ A ]}{Δ t} = - \frac{1}{m _{2}} \frac{Δ [ B ]}{Δ t} = + \frac{1}{n _{1}} \frac{Δ [ C ]}{Δ t} = + \frac{1}{n _{2}} \frac{Δ [ D ]}{Δ t}$

Consider the chemical reaction,

$N_{2} (g) + 3 H_{2} (g) \to 2 NH_{3} (g)$

The rate of reaction may be expressed as:

Options:

Answer:

Solution:

$N_{2} (g) + 3 H_{2} (g) \to 2 NH_{3} (g)$

$- \frac{d [ N _{2} ]}{dt} = - \frac{1}{3} \frac{d [ H _{2} ]}{dt} = + \frac{1}{2} \frac{d [ NH _{3} ]}{dt} = Rate of reaction.$

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

⏱ 2mℹ️ Source: QB

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