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) $2 \mathrm{O}_{3}(\mathrm{g}) \longrightarrow 3 \mathrm{O}_{2}(\mathrm{g})$ (b) $2 \mathrm{HOF}(\mathrm{g}) \longrightarrow 2 \mathrm{HF}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g})$

Give the relative rates of disappearance of reactants and formation of products for each of the following reactions.
(a) $2 \mathrm{O}_{3}(\mathrm{g}) \longrightarrow 3 \mathrm{O}_{2}(\mathrm{g})$
(b) $2 \mathrm{HOF}(\mathrm{g}) \longrightarrow 2 \mathrm{HF}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g})$

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Key Concepts

Stoichiometry

Stoichiometry refers to the quantitative relationships in a chemical reaction as expressed by the coefficients in the balanced equation. It determines the proportional amounts of reactants consumed and products formed, allowing us to relate the change in quantities of one substance to that of another.

Relative Reaction Rates

Relative reaction rates are derived from the stoichiometric coefficients and indicate how fast reactants disappear or products form compared to the overall progress of the reaction. The rate of change in concentration for a particular species is proportional to its coefficient in the balanced equation, with all rates being expressed in relation to a common reaction rate.

Disappearance and Formation Rates

The rates at which reactants disappear and products form are directly linked to the reaction’s stoichiometry. Specifically, for each species involved, the observed rate is the product of its stoichiometric coefficient and the overall rate of the reaction, adjusted by a negative sign for reactants (disappearance) and a positive sign for products (formation).

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