a. Carbon monoxide and nitrogen dioxide react to form carbon dioxide and nitric
ID: 571856 • Letter: A
Question
a. Carbon monoxide and nitrogen dioxide react to form carbon dioxide and nitric oxide. A series of experiments were performed to gain understanding of the kinetics of the reaction.
1. The sum of the coefficients in the balanced reaction equation is:
(hint: type in the number. Do not spell the work for the number, i.e. "1" not "one")
2. In the reaction described in question a, the reaction order with respect to nitrogen dioxide is:
(hint: simply type in a number. Do not type 0th order, 1st order 2nd order, one-half order, etc.)
3. In the reaction described in question a, the average rate constant, including the correct units for k, is:
4. In the reaction described in question a , the rate law for the reaction is:
CO] (M) [NO2] (M) initial rate (M/s) 5.1 x 10^-4 0.35 x 10^-4 3.4 x 10^-8 5.1 x 10^-4 0.70 x 10^-4 6.8 x 10^-8 5.1 x 10^-4 0.18 x 10^-4 1.7 x 10^-8 1.0x 10^-3 0.35 x 10^-4 6.8 x 10^-8 1.5 x 10-3 0.35 x 10-4 10.2 x 10-8Explanation / Answer
1) CO + NO2 -----------> CO2 + NO reaction is balanced
sum of the coefficients = 1 + 1 + 1 + 1 = 4
2) when NO2 is doublled rate also doublled so with respect to NO2 order = 1
order with respect to NO2 = 1
3) rate = K [CO][NO2]
K = rate / [CO][NO2]
K = 3.4 x 10-8 / [5.1 x 10-4][0.35 x 10-4]
K = 3.4 x 10-8 / 1.785 x 10-7
K = 1.90 x 10-1 M-1s-1
4) rate law as follows
rate = K [CO][NO2]
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