1)
Molar mass of O2 = 32 g/mol
mass(O2)= 3.94 g
use:
number of mol of O2,
n = mass of O2/molar mass of O2
=(3.94 g)/(32 g/mol)
= 0.1231 mol
Given:
V = 8.22 L
n = 0.1231 mol
T = 76.0 oC
= (76.0+273) K
= 349 K
use:
P * V = n*R*T
P * 8.22 L = 0.1231 mol* 0.08206 atm.L/mol.K * 349 K
P = 0.4289 atm
Answer: 0.429 atm
2)
1st find partial pressure of Xe
Molar mass of Xe = 131.3 g/mol
mass(Xe)= 17.0 g
use:
number of mol of Xe,
n = mass of Xe/molar mass of Xe
=(17 g)/(1.313*10^2 g/mol)
= 0.1295 mol
Given:
V = 8.22 L
n = 0.1295 mol
T = 76.0 oC
= (76.0+273) K
= 349 K
use:
P * V = n*R*T
P * 8.22 L = 0.1295 mol* 0.08206 atm.L/mol.K * 349 K
P = 0.451 atm
Now use:
Total pressure = p(Xe) + p(O2)
= 0.451 atm + 0.429 atm
= 0.880 atm
Answer: 0.880 atm
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