Question

One-tenth kmol of carbon monoxide (CO) in a piston-cylinder assembly undergoes a process from P1-150 kPa, T1-300 K to P2-500 kPa, T2-370 K. For the process, W--300 kJ. Employing the ideal gas model, determine a.) the heat transfer, in kJ, b.) the change in entropy, in kJ/K. c.) Show the process on a sketch of the T - s diagram.

Answer 1

To find the heat transfer, use the First Law of Thermodynamics. To find the change in entropy, use the ideal gas equation.

Step-by-step explanation:

In this problem, we are given the initial and final values of pressure and temperature for CO in a piston-cylinder assembly, as well as the work done during the process. We are asked to determine the heat transfer and change in entropy for the process.

To find the heat transfer, we can use the First Law of Thermodynamics: Q = ΔU + W, where Q is the heat transfer, ΔU is the change in internal energy, and W is the work done. Since we are not given the initial or final internal energy values, we can rearrange the equation to solve for Q: Q = W - ΔU.

To find the change in entropy, we can use the ideal gas equation: ΔS = n * R * ln(V2/V1) + n * R * ln(T2/T1), where ΔS is the change in entropy, n is the number of moles, R is the ideal gas constant, V1 and V2 are the initial and final volumes, and T1 and T2 are the initial and final temperatures.

Using the given values, we can calculate the heat transfer and change in entropy for the process.