The oxidation of ammonia in air is catalysed by platinum...

The oxidation of ammonia in air is catalysed by platinum metal \[ 4 \mathrm{NH}_{3}(\mathrm{g})+5 \mathrm{O}_{2}(\mathrm{g}) \rightarrow 4 \mathrm{NO}(\mathrm{g})+6 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \] Write an expression for the rate of reaction in terms of differentials for the consumption of the reactants and formation of the products. (Sections $9.2 \text { and } 9.4)$

The oxidation of ammonia in air is catalysed by platinum metal
\[
4 \mathrm{NH}_{3}(\mathrm{g})+5 \mathrm{O}_{2}(\mathrm{g}) \rightarrow 4 \mathrm{NO}(\mathrm{g})+6 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})
\]
Write an expression for the rate of reaction in terms of differentials for the consumption of the reactants and formation of the products. (Sections $9.2 \text { and } 9.4)$

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Key Concepts

Stoichiometry in Rate Equations

Stoichiometric coefficients from the balanced chemical equation are used to relate the rates of consumption or formation of different species. When writing the rate expression, the changes in concentration of each reactant or product are divided by their respective stoichiometric coefficients to ensure the rate is consistent across all components of the reaction.

Rate of Reaction

The rate of reaction is a measure of how quickly reactants are converted into products over time. It is typically expressed in terms of changes in concentration or pressure per unit of time, and it can be applied to both the consumption of reactants and the formation of products in a chemical reaction.

Differential Rate Expression

A differential rate expression represents the rate of change of concentration (or partial pressure) with respect to time, using infinitesimal changes. This approach formulates the reaction rate as a derivative, such as d[Reactant]/dt or d[Product]/dt, which quantifies the instantaneous rate at which species are consumed or produced.

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