SUMMARY
The discussion focuses on calculating the change in internal energy (dU) of two moles of carbon monoxide (CO) during an adiabatic compression from a volume of 30 liters to 10 liters at an initial pressure of 1.2 atm. The relevant equations include the first law of thermodynamics, Q = dU + W, and the ideal gas law, PV = nRT. The specific heat capacity at constant pressure (Cp) is given as 29.16 J/(mol * K). The solution requires determining the initial temperature (T1) and the final temperature (T2) using the adiabatic process equation TV^γ = constant.
PREREQUISITES
- Understanding of the ideal gas law (PV = nRT)
- Knowledge of adiabatic processes and the equation TV^γ = constant
- Familiarity with the first law of thermodynamics (Q = dU + W)
- Concept of specific heat capacity (Cp) for gases
NEXT STEPS
- Calculate initial temperature (T1) using the ideal gas law with given pressure and volume
- Determine final temperature (T2) using the adiabatic process equation TV^γ = constant
- Calculate work done (W) during the adiabatic compression
- Compute the change in internal energy (dU) using dU = nCpdT
USEFUL FOR
Students studying thermodynamics, particularly those focusing on gas laws and energy transformations in adiabatic processes.