Final answer:
The reaction rate of the equation 2 N2O (g) → 2 N2 (g) + O2 (g) can be expressed by considering the rate of disappearance of the reactant N2O and the formation rates of the products N2 and O2, taking into account their stoichiometric coefficients in the balanced equation.
Step-by-step explanation:
When considering the reaction rate of the equation 2 N2O (g) → 2 N2 (g) + O2 (g), we look at how the concentrations of reactants and products change over time. For reactants, the rate is negative because their concentration decreases, and for products, it is positive.
To express the reaction rate with respect to each of the reactants and products, we use the stoichiometry of the balanced equation. The rate of disappearance of N2O is written as -Δ[N2O]/Δt, and because two moles of N2O form two moles of N2 and one mole of O2, the rate of formation of N2 is Δ[N2]/Δt, which is the same as the rate of disappearance of N2O. However, for O2, since only one mole is produced, the rate of formation is Δ[O2]/Δt, which is half the rate of the disappearance of N2O when the stoichiometry and coefficients are taken into account. Hence, the reaction rate can be expressed as:
- Rate with respect to N2O: -Δ[N2O]/Δt
- Rate with respect to N2: Δ[N2]/Δt
- Rate with respect to O2: Δ[O2]/Δt = (-1/2) (Δ[N2O]/Δt)