When you assume that the gas is behaving ideally, the gas molecules are very far from each other that they do not have any intermolecular forces. If it behaves this way, you can assume the ideal gas equation:
PV = nRT, where
P is the pressure
V is the volume
n is the number of moles
R is a gas constant
T is the absolute temperature
When the process goes under constant pressure (and assuming same number of moles),
P/nR = T/V = constant, therefore,
T₁/V₁=T₂/V₂
If V₂ = V₁(1+0.8) = 1.8V₁, then,
T₂/T₁ = 1.8V₁/V₁
Cancelling V₁,
T₂/300=1.8
T₂ =540 K
If you do not assume ideal gas, you use the compressibility factor, z. The gas equation would now become
PV =znRT
However, we cannot solve this because we don't know the value of z₁ and z₂. There will be more unknowns than given so we won't be able to solve the problem. But definitely, the compressibility factor method is more accurate because it does not assume ideality.
Answer:
See explanation
Explanation:
From the information provided;
P1 = initial pressure = 758.0 mmHg
T1 = Initial temperature = 32.7°C + 273 = 305.7 K
V1 = Initial volume?
P2 = Final pressure = 364.2 mmHg
V2 = Final volume = 425 L
T2= Final Temperature = 3.10°C + 273 = 276.1 K
P1V1/T1 = P2V2/T2
P1V1T2 =P2V2T1
V1 = P2V2T1/P1T2
V1 = 364.2 * 425 * 305.7/758.0 * 276.1
V1 = 226. 18 L
B) Total pressure = 100.0 kPa
Pressure of Helium = 83.1 kPa
Pressure of carbon dioxide = 0.1000 kPa
Pressure of oxygen ?
From Dalton's law of partial pressures;
PT = P1 + P2 +P3 +.........
Hence;
Poxygen = 100.0 kPa - (83.1 kPa + 0.1000 kPa)
Poxygen = 16.8 kPa
Answer: Link in Explaination will help you!! :)
Explanation: https://otherhalf.life/image.php?id=IYZMDN.pdf
