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We’re being asked to determine the rate of disappearance of O2.
We are given the balanced equation for the reaction:
2 NO(g) + O2 (g) → 2 NO2 (g)
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 reaction 2NO(g) + O2 (g) → 2NO2 (g) is second order in NO and first order in O2. When [NO]= 4.1×10−2 M and [O2]= 3.6×10−2 M , the observed rate of disappearance of NO is 9.3×10−5 M/s .
What is the rate of disappearance of O2 at this moment?
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Based on our data, we think this problem is relevant for Professor Tyson's class at UMASS.