Question

Please answer all three parts and show work. Thank you!

1. An ideal gas assumes molecules are point particles and do not interact with each other. In reality, molecules occupy space! To correct for this, the ideal gas equation of state is adjusted to take the volume occupied by the molecules into account for a real gas: PV = nRT or P = nRTV is modified to P = nRT/(V-nb) (IDEAL GAS) (REAL GAS Where "b" is related to the volume occupied by 1 mol of molecules. As expected, b will be different for H2, in comparison to propane. Let's take a value of "b" 4x105 m3 /mol, which is average for small diatomic molecules. 1. 1 mol of a real diatomic gas at 200K is compressed from a total volume of 0.3L to 0.1L: (a) Calculate the work done if the process is carried out isothermally and reversibly. (b) Calculate the change in entropy of the real gas when compressed isothermally. (c) Would the work done be the same if the gas was compressed between the same initial and final states as in (a), but at constant pressure? Explain, without necessarily doing a calculation.

Answer 1

C sas ot mo o m/ma hwly and Yomsbly (-nb) V 01L (v-wb) 0 3 ー-g@3314X 2dV [In (0-1-41副

2-6x 2.6 Fn sumal process mdle

x240 8.3 lux 20D丁 h1 3 lad -3 wak done