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We’re given the balanced reaction:
2 NO(g) + 2 H2(g) → 2 H2O(g) + N2(g)
We’re being asked to calculate the average rate of the reaction with respect to N2 and H2O given that Δ[NO]/Δt = –19.0 M/s. Recall that the average rate of a reaction is given by:
where Δ[A] = change in concentration of reactants or products (in mol/L or M) and Δtime = change in time. We can simply do a rate-to-rate comparison based on the stoichiometric coefficients.
The gas NO reacts with H2, forming N2 and H2O:
2NO (g) + 2H2 (g) → 2H2O (g) + N2 (g)
If Δ[NO]/Δt = -19.0 M/s under a given set of conditions, what are the rates of change of [N 2] and [H2O]?
Rate of change of [N2]:
Rate of change of [H2O]:
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