using the ideal gas equation
PV =nRT
n = mass / molar mass
PV = mass * R T / molar mass
=> mass = PV * molarmass / RT
P = 3.12 atm
V = 6.88 L
R = 0.0821 L atm / k mol
T = 62.5 c = 335.5 K
molar mass = 83.798 g/mol
mass = 3.12 * 6.88 * 83.798 / 0.0821 * 335.5
mass => 65.3 grams
=> no of moles = mass / molar mass
for Ar = 4.05g / 39.948 g/mol => 0.1014 moles
V = 2.00 L
R = 0.0821 l atm /k mol
T = 27c = 300 k
using the ideal gas equation PV = nRT
P = nRT / V
P = 0.1014 * 0.0821 * 300 / 2
Partial pressure of Ar = 1.2485 atm
partial pressure of He = 2.85 atm
total pressure = Partial pressure of Ar + partial pressure of He => 1.2485 + 2.85 => 4.098 atm
answer => 4.1 atm
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