1 mol of a gas occupies a volume of 5L at 600K and 3atm. Which of the following statements regarding it is/are correct? (use R=0.08atmL/molK )
I. The compressibility factor Z for the gas is .
II. The volume occupied by the gas at same temperature and pressure will be less than that occupied by an ideal gas.
III. The gas shows positive deviation
Answers
Answer:
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Answer: The compressibility of gas is 0.3125
Explanation:
Given: Mole, n = 1mol
Volume, V = 5L
Temprature, T= 600K
Pressure, P = 3atm
We know,
Compressibility factor, (Z) = PVreal/nRT
where, P = Pressure (in atm)
Vreal = Volume of real gas (in L)
n = number of mole
T = temperature
R = 0.0821 atm-L/mol-K
So, Z = PVreal/nRT = 3 × 5/1 × 0.08 × 600 = 0.3125.
Compressibility factor of the gas is 0.3125
The compressibility factor of natural gas (which corrects for the ratio of actual volume to ideal volume) is roughly an 0.5% correction in volume per 100 psi of pressure for an orifice meter under normal pressure and temperature conditions. Hence, an error of several percent in the compressibility factor only produces a small error in volume. However, if the gas is near its critical point, correction factors of as much as 225% are required, and small errors in measured variables (temperature and pressure) are reflected as large errors in volume. These values are doubled for non-head meters.
Likewise, gases with large concentrations of non-hydrocarbon gases in their compositions are not as difficult to calculate as accurately, since new data are available from the AGA on these mixtures. Some of the theoretical values obtained by the pseudocritical method (based on the mixture composition) have shown errors of several percent when compared with empirically determined test data on the same gas. This problem becomes more pronounced as the percentage of methane is reduced. If the value of the product handled is sufficient, then actual compressibility tests are recommended to confirm that the calculated data complies with the tolerances required.
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