Problem: 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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FREE Expert Solution

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:


Rate = [A]time


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 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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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Average Rate of Reaction concept. You can view video lessons to learn Average Rate of Reaction. Or if you need more Average Rate of Reaction practice, you can also practice Average Rate of Reaction practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Tyson's class at UMASS.