Question
Rate equation is r=k[A]^n[B]^m
A prevalent form of toxic pollutant NO x formed in power-plant combustors is NO. Under favorable conditions. NO can be decomposed ("reduced") via the following reaction: 2NO rightarrow N2 + O2 At 1620 K. for a reaction rate expressed in gmol/L s and the amount of NO expressed in atmospheres, the reaction rate constant for this irreversible reaction is 0.0108 gmol/L s (atm)2 (from reference 2. p. 813). Assuming that NO is the only reactant, use the units of the rate constant to determine the order of this reaction in terms of NO. If a reactor is designed to reduce NO at a rate of 0.056 gmol/min L at 1620 K. what partial pressure of NO is needed in the reactor?
Explanation / Answer
a)
units balancing
rate of rxn= K * (atm)^p
gmol/L s=gmol/[L s (atm)^2] *(atm)^(p)
p=2
So the reaction is second ordered reaction
b)
