NO2 reacts with F2 in the gas phase according to the folowing chencial equation: 2NO2(g)+F2(g)2NO2F(g) It is observed that, when the conceetration of F2 is reduced to 1/4 of its initial value, the rate of the reaction is also reduced to 1/4 of ita initial value. When the concentration of NO 2 is multiglied by 3.41, the rate of the reaction alse increases by a factor of 3.41. (a) Write the rate expression for this reaction, and give the uniss of the rate constant k, assuming concentration is expressed as mol L4 and time is in seconds. rate=kunta= (b) It (NO2) were mutiplied by 3.64 and (F2) by 2.09, what change in the rate would be observed? The rate would increate by a fector of