T₁ = 50,14 K.
p₁ = 258,9 torr.
T₂ = 161,2 K.
p₂ = 277,5 torr.
R = 8,314 J/K·mol.
Using Clausius-Clapeyron equation:
ln(p₁/p₂) = - ΔHvap/R · (1/T₁ - 1/T₂).
ln(258,9 torr/277,5 torr) = -ΔHvap/8,314 J/K·mol · (1/50,14 K - 1/161,2 K).
-0,069 = -ΔHvap/8,314 J/K·mol · (0,0199 1/K - 0,0062 1/K).
0,0137·ΔHvap = 0,573 J/mol.
ΔHvap = 41,82 J.
Answer:
n = 11.45 mol
Explanation:
Given data:
Number of moles = ?
Volume of gas = 98 L
Pressure = 2.8 atm
temperature = 292 K
Solution:
The given problem will be solve by using general gas equation,
PV = nRT
P= Pressure
V = volume
n = number of moles
R = general gas constant = 0.0821 atm.L/ mol.K
T = temperature in kelvin
2.8 atm × 98 L = n × 0.0821 atm.L/ mol.K × 292 K
274.4 atm.L = n × 23.97atm.L/ mol
n = 274.4 atm.L /23.97atm.L/ mol
n = 11.45 mol
Answer:
B mixture can be separated by physical means
