USA: +1 725-224-8795 
Sign in
If 1.65 moles of argon and 1.63 moles of oxygen are placed in a 14.3 L container at 45°C, what is the pressure of the mixture in atmospheres? Add 273 to convert to Kelvin. R = 0.0821 L atm/mol K Report your answer in atm to three significant figures.
Expert Answer
Apply ideal gas law
Don't use plagiarized sources. Get Your Custom Essay on
Question & Answer: If 1.65 moles of argon and 1.63 moles of oxygen are placed in a 14.3 L container at 45°C, what is…..
GET AN ESSAY WRITTEN FOR YOU FROM AS LOW AS $13/PAGE
total mol = 1.65 + 1.63 = 3.28 moles of total mix
Apply Ideal Gas Law,
PV = nRT
where
P = absolute pressure
V = total volume of gas
n = moles of gas
T = absolute Tmperature
R = ideal gas constant
PV = nRT
P = nRT/V
P = (3.28 mol )(0.082 Latm/molK)(45+273 K ) / (14.3 L)
P = 5.9810 atm
to 3 sig fig:
P = 5.98 atm
