Give the relative rates of disappearance of reactants and...

Give the relative rates of disappearance of reactants and formation of products for each of the following reactions. (a) $2 \mathrm{NO}(\mathrm{g})+\mathrm{Br}_{2}(\mathrm{g}) \longrightarrow 2 \mathrm{NOBr}(\mathrm{g})$ (b) $\mathrm{N}_{2}(\mathrm{g})+3 \mathrm{H}_{2}(\mathrm{g}) \longrightarrow 2 \mathrm{NH}_{3}(\mathrm{g})$

Give the relative rates of disappearance of reactants and formation of products for each of the following reactions.
(a) $2 \mathrm{NO}(\mathrm{g})+\mathrm{Br}_{2}(\mathrm{g}) \longrightarrow 2 \mathrm{NOBr}(\mathrm{g})$
(b) $\mathrm{N}_{2}(\mathrm{g})+3 \mathrm{H}_{2}(\mathrm{g}) \longrightarrow 2 \mathrm{NH}_{3}(\mathrm{g})$

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Key Concepts

Reaction Rate

The reaction rate is defined as the change in concentration of a reactant or product per unit time. It quantifies how fast a reaction occurs and can be expressed in terms of the rate at which reactants disappear or products form. This rate must be consistent when expressed for all species involved, taking into account their stoichiometric coefficients.

Stoichiometric Coefficients

In a balanced chemical equation, the stoichiometric coefficients indicate the proportion in which reactants and products participate in the reaction. They are used to relate the changes in concentration of each species to a common reaction rate. For example, if a reactant has a coefficient of 2, its rate of disappearance will be twice the overall reaction rate, when adjusted for the coefficient.

Relative Rate Formulation

To relate the rates of change of each reactant or product in a chemical reaction, the rate of disappearance or formation is divided by its respective stoichiometric coefficient. This ensures that the relative rates are normalized and consistent across all species in the reaction, allowing for meaningful comparison among them.

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