Finding Partial Pressures?
Ozone completely reacts with NO, producing NO2 and O2. A 16.2 L vessel is filled with 0.802 mol of NO and 0.802 mol of O3 at 494.0 K. Find the partial pressure of each product and the total pressure in the flask at the end of the reaction.
1) P NO2 = ? atm
2) P O2 = ? atm
3) P total = ? atm
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PV = nRT
P = pressure in atmospheres
V = volume in liters
n = number of moles
R = gas constant (of when pressure is in atmospheres)
T = temperature in Kelvin
moles of NO2: Everything is a one to one reaction, so 0.802 mol of NO2
moles of O2: same as NO2
Pressure of NO2: (P)*(16.2L) = (0.802 mol)*(0.08206 atm L/mol K)*(494.0K)
P = 2.006 atm
Pressure of O2: (P)*(16.2L) = (0.802 mol)*(0.08206 atm L/mol K)*(494.0K)
P = 2.006 atm
Total Pressure: P = 4.01 atm