Problem: 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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FREE Expert Solution
FREE Expert Solution

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.


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Problem Details

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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