Ammonia is manufactured in large amounts by the reaction N2(g)+3 H2(g) ⟶2 NH3(g) (a) How is the

step 1 The balanced chemical reaction is provided where one mole of N2 gas reacts with three moles of H

Ammonia is manufactured in large amounts by the reaction...

Ammonia is manufactured in large amounts by the reaction $$\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)$$ (a) How is the rate of consumption of $\mathrm{H}_{2}$ related to the rate of consumption of $\mathrm{N}_{2}$ ? (b) How is the rate of formation of $\mathrm{NH}_{3}$ related to the rate of consumption of $\mathrm{N}_{2}$ ?

Ammonia is manufactured in large amounts by the reaction
$$\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)$$
(a) How is the rate of consumption of $\mathrm{H}_{2}$ related to the rate of consumption of $\mathrm{N}_{2}$ ?
(b) How is the rate of formation of $\mathrm{NH}_{3}$ related to the rate of consumption of $\mathrm{N}_{2}$ ?

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Key Concepts

Stoichiometric Relationships in Reaction Rates

Stoichiometric relationships link the rates of consumption and formation of species in a chemical reaction based on their coefficients in the balanced equation. For instance, the change in the concentration of one reactant can be related to the change in another by dividing or multiplying by their respective stoichiometric coefficients, ensuring that the overall reaction proceeds consistently with the balanced chemical equation.

Balanced Chemical Equation

A balanced chemical equation not only represents the substances involved in a chemical reaction but also shows the stoichiometric coefficients that indicate the relative molar amounts of reactants and products. These coefficients are crucial because they provide the direct proportionality factors used to relate the rates at which different species are consumed or produced during the reaction.

Reaction Rate

The reaction rate quantifies how quickly the concentrations of reactants decrease or the concentrations of products increase over time. In chemical kinetics, this rate is typically expressed in terms of concentration per unit time, and its calculation often involves the use of negative signs for reactants (indicating consumption) and positive signs for products (indicating formation).

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