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Assuming your natural gas is 100% methane, the specific heat at constant pressure at 25°C:
Cp/R = 4.217
where R is the ideal gas constant represented in terms of energy.
Using R=8.314 Joule/(Kelvin*mole)
This yields Cp=35.06 J/(K*mol)
The heat capacity at constant volume, Cv, is related to the heat capacity at constant pressure, Cp by the following expression:
Cp-Cv=R
Therefore Cv=Cp-R = 35.06 J/(K*mol) - 8.314 J/(K*mol) = 26.75 J/(K*mol)
Assumptions:
- The system is a monotonic ideal gas
- The temperature is at or near 25°C
- Heat capacity is not a function of temperature
A more accurate heat capacity as a function of temperature is
Cp/R = 1.702 + 9.081E-3*T - 2.164*T^(-2)
where T is in Kelvins from 298K (25°C) to 1500K (1226.85°C)
Assumptions 2 and 3 above do not apply to this.
Source: Introduction to Chemical Engineering Thermodynamics. 7th Ed. by J.M. Smith, Appendix C p. 684
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Air expands according to the law pv1.3 a constant inside an enclosed cylinder find its specific heat?
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