Ozone reacts completely with NO, producing NO2 and O2. A 13.0 L vessel is filled with 1.30 mol of NO and 1.30 mol of O3 at 401.0 K. Find the partial pressure of each product and the total pressure in the flask at the end of the reaction.

6.58 atm total

3.29 atm NO2

3.29 atm O2

Explanation:

Balanced equation:

O3 + NO → NO2 + O2

There are equal numbers of moles of both reactants, so neither is in excess and either could be considered the limiting reactant.

(1.30 mol NO) x (1 mol NO2 / 1 mol NO) = 1.30 mol NO2

(1.30 mol NO) x (1 mol O2 / 1 mol NO) = 1.30 mol O2

Total pressure by using the formula;

P = nRT / V

= (1.30 mol + 1.30 mol) x (0.08205746 L atm/K mol) x (401.0 K) / (13.0 L)

= 6.58 atm

Partial pressure for NO2;

(6.58 atm) x (1.30 mol NO2) / (1.30 mol + 1.30 mol)

= 3.29 atm NO2

Partial pressure for O2

6.58 atm total - 3.29 atm NO2

= 3.29 atm O2