1. In studying the reaction: the initial Concentration of N2O5 was 0.64 mol/L. A

Question

1. In studying the reaction: the initial Concentration of N2O5 was 0.64 mol/L. After 30 minutes into, the reaction, all the N2O5 has reacted. a. What is the average rate of the reaction in the time interval of 30 minutes? b. Is it correct to assume, based on the balanced equation, the rate equation is: Rate = k[N2O5]^2 c. Suppose the reaction rate is determined by measuring the rate of decreased of N2O5 concentration,-Delta(N2O5)/deltat, and simultaneously by the rate of increase of NO2 concentration, which rate will come out higher and by what factor?

Explanation / Answer

1 (a) 2N2O5(g) = 4NO2 + O2

initial concen = o.64 mol/l, final conc = 0,

average concentration = change in concentration /time = 0.64-0/30 = 0.021 mol/L*min

(b) it is correct ie rate = K[N2O5}2, if it is unimolecular reaction.

(c) 2N2O5(g) = 4NO2(g) + O2(g)

-rN2O5/2 = rNO2/4 = rO2

so -rN2O5 = rNO2/2

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