n Ne = grams/molar mass = ?
n Aar = grams/molar mass = ?
Then PV = mRT and use n Ne to solve for pNe. Use n for Ar to solve for pAr.
A gas mixture in a 1.55L at 298K container contains 10.0g Ne and 10.0g Ar. Calculate the partial pressure " in atm" of Ne and Ar in the container
2 answers
10.0 g Ne / 20.18 g/mol = 0.496 mol
P*1.55 L = 0.496 mol * 0.08206 L*atm/mol*K * 298 K
P of Ne = 7.82 atm
10.0 g Ar / 39.948 g/mol = 0.25 mol
P*1.55 L = 0.25 mol * 0.08206 L*atm/mol*K * 298 K
P of Ar = 3.94 atm
P*1.55 L = 0.496 mol * 0.08206 L*atm/mol*K * 298 K
P of Ne = 7.82 atm
10.0 g Ar / 39.948 g/mol = 0.25 mol
P*1.55 L = 0.25 mol * 0.08206 L*atm/mol*K * 298 K
P of Ar = 3.94 atm
2 answers