In: Chemistry
a 2.00 l container holds 4.00 moles of o2 and 2.70 moles of he at 293 k. What is the partial pressure of o2? He? what is the total pressure?
Ideal gas equation
PV = nRT where, P = atm pressure= ?
V = volume in Liter = 2 L
n = number of mole = 4.00 + 2.70 = 6.70
R = 0.08205L atm mol-1 K-1 =Proportionality constant = gas constant,
T = Temperature in K = 293 K
We can write ideal gas equation
P = nRT/V
Substitute value in above equation
P = 6.700.08205
293
/ 2 = 80.536 atm
Total pressure = 80.536 atm
total mole = 4.00 + 2.70 = 6.70
mole fraction of O2 = 4/6.70 = 0.597
mole fraction of He = 2.70/6.70 = 0.403
Pi = Xi P where,
Pi = partial pressure of indivisual gas, P = total
pressure, Xi = mole fraction of indivisual gas
substiture value in above equation
Partial pressure of O2 = 0.597
80.536 = 48.079992 atm
Partial pressure of He = 0.403 80.536 =
32.456008 atm