Concept explainers
The mass fractions of a mixture of gases are 15 percent nitrogen, 5 percent helium, 60 percent methane, and 20 percent ethane. Determine the mole fractions of each constituent, the mixture’s apparent molecular weight, the partial pressure of each constituent when the mixture pressure is 1200 kPa, and the apparent specific heats of the mixture when the mixture is at the room temperature.
The mole fraction of
The mole fraction of
The mole fraction of
The mole fraction of
The apparent molecular weight of the mixture.
The partial pressure of
The partial pressure of
The partial pressure of
The partial pressure of
The constant-pressure specific heat of the mixture,
The constant-volume specific heat,
Answer to Problem 32P
The mole fraction of
The mole fraction of
The mole fraction of
The mole fraction of
The apparent molecular weight of the mixture is
The partial pressure of
The partial pressure of
The partial pressure of
The partial pressure of
The constant-pressure specific heat of the mixture,
The constant-volume specific heat,
Explanation of Solution
Refer to Table A-1, Obtain the molar masses of
Refer to Table A-2a, obtain the constant-pressure specific heats of the gases at room temperature.
Write the mole number of
Here, the mass of nitrogen gas is
Write the mole number of
Here, the mass of helium gas is
Write the mole number of
Here, the mass of methane gas is
Write the mole number of
Here, the mass of ethane gas is
Write the equation to calculate the mole number of the mixture.
Write the formula to calculate the mole fraction of
Write the formula to calculate the mole fraction of
Write the formula to calculate the mole fraction of
Write the formula to calculate the mole fraction of
Calculate the molar mass of the gas mixture.
Write the partial pressure of
Here, mixture pressure is
Write the partial pressure of
Write the partial pressure of
Write the partial pressure of
Write the equation to calculate the constant-pressure specific heat of the mixture.
Here, mass fraction of
Calculate the gas constant of the mixture.
Here, the universal gas constant is
Calculate the constant volume specific heat.
Conclusion:
Substitute 15 kg for
Substitute 50 kg for
Substitute 50 kg for
Substitute 20 kg for
Substitute
Substitute
Thus, the mole fraction of
Substitute
Thus, the mole fraction of
Substitute
Thus, the mole fraction of
Substitute
Thus, the mole fraction of
Substitute 100 kg for
Thus, the apparent molecular weight of the mixture is
Substitute 0.08637 for
Thus, the partial pressure of
Substitute 0.08637 for
Thus, the partial pressure of
Substitute 0.6046 for
Thus, the partial pressure of
Substitute 0.1075 for
Thus, the partial pressure of
Substitute 0.15 for
Thus, the constant-pressure specific heat of the mixture,
Substitute
Substitute
Thus, the constant-volume specific heat,
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Chapter 13 Solutions
Thermodynamics: An Engineering Approach
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