2 NO(g) + O2(g) → 2 NO2(g) Suppose that at a particular moment during the reaction nitric oxide (NO) is reacting at the rate of 0.070 M/s. (a) At what rate is NO2 being formed? (b) What rate is molecular oxygen reacting?

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Answer 1 · 2018-02-05T17:01:42

Consider,

$2NO(g) + O_2(g) to 2NO_2(g)$

Moreover, understand that reaction rates are proportional to the stoichiometry of the reaction. Hence,

$(0.070M)/s * (2NO_2)/(2NO) = (0.070M)/s$

is the rate of appearance of nitrogen dioxide, and

$(0.070M/s) * (O_2)/(2NO) = (-0.035M)/s$

is the rate of disappearance of the oxygen.

To be sure, reaction rates are merely,

$(Delta[A])/(Deltat)$

and the concentrations of the constituents are proportional to the stoichiometry.

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