Question

NO2 reacts with CO in the gas phase according to the following chemical equation: NO2(g) +CO(g)CO2(g) +NO(g) It is observed that, when the concentration of CO is reduced to 1/4 of its initial value, the rate of the reaction is does not change. When the concentration of NO2 is multiplied by 3.61, the rate of the reaction increases by a factor of 13.0.

(a) Write the rate expression for this reaction, and give the units of the rate constant k, assuming concentration is expressed as mol L-1 and time is in seconds. rate = k units =

(b) If [NO2] were multiplied by 3.45 and [CO] by 3.74, what change in the rate would be observed? The rate would increase by a factor of

Answer 1