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Recall that for a reaction aA → bB, the rate of a reaction is given by:
We can simply do a rate-to-rate comparison based on the stoichiometric coefficients.
Reaction: dinitrogen monoxide → nitrogen and oxygen
Reaction: 2 N2O(g) → 2 N2(g) + O2(g)
Since N2O is a reactant, the rate should be negative since reactants are used up/consumed.
Dinitrogen monoxide decomposes into nitrogen and oxygen when heated. The initial rate of the reaction is 2.4 × 10−2 M/s. What is the initial rate of change of the concentration of N2O (that is, Δ[N2O]/Δt)?
2 N2O(g) → 2 N2(g) + O2(g)
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