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 would happen to the rate if the concentration of NO were increased by a factor of 2.1?

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We are asked what would happen to the rate if the concentration of NO were increased by a factor of 2.1


Calculate the rate constant, k: 

rate = k[NO]2[O2] k = rate[NO]2[O2]  k = 9.3×105  M/s[4.1×102 M]2[3.6×102 M] 

k = 1.54 M-2 s-1 


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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 would happen to the rate if the concentration of NO were increased by a factor of 2.1?

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