Please find the attachment.![prove [cp-CV=R [cv = 8/12-1)] [cp = YR/(1-1) де кто о #ket, HEU + PV foạide91 995 je pv=nRT H=ut MRT Whene, Differenciate bot](http://img.homeworklib.com/questions/7675a180-2872-11ec-be06-6b74314e285e.png?x-oss-process=image/resize,w_560)
![put cp = Y Cv in equation ③ anny y cy - Cv=R CV (Y-1) =R [cv = 2 ] -](http://img.homeworklib.com/questions/77227a80-2872-11ec-a4fe-2bd49decb627.png?x-oss-process=image/resize,w_560)
Useful constant: R-0.08315L.bar/K.mol, 0.08206L.atm/K.mol or 8.314J/K.mol, Cv(any monoatomic gas) 3R/2 and Cp-Cv+ R for an ideal gas. Section I 1. Assuming that CO2 is an ideal gas, calculate ASo (in the unit, J K:1) for the following process 1 CO (g, 298 K, 1 bar) 1 CO (g, 1000 K, 1 bar) Given that: Cv 18.334 + 42.262 x 103 T - 142.4 x 10-7 T2 (where Cv is in of JK-1)
One mole of an ideal gas with CP = (7/2)R and CV = (5/2)R expands from P1 = 8 bar and T1 = 630 K to P2 = 1 bar. Take the value of R as 8.314 J·mol-1·k-1. At constant volume (assume mechanical reversibility), find the value of W, Q, ΔU, and ΔH? rt.)
2. One mole of an ideal gas, CP - (7/2)R and CV - (5/2)R, is compressed adiabatically in a piston/cylinder device from 2 bar and 25°C to 7 bar. The process is irreversible and requires 35% more work than a reversible, adiabatic compression from the same initial state to the same final pressure. What is the entropy change of the gas?
Consider a reversible adiabetic compression of an ideal gas with CV,m = 3R/2 and CP,m = 5R/2. 3.0 mol of this ideal gas with a volume of 30.0 L changes from an initial temperature of 300 K to a final temperature of 600 K. For this process, compute the final volume.
A. Compute Cp-Cv for a gas described by the equation of state p= RT/V-b B. For this equation of state, does a measurement of Cp-Cv reveal non-ideal behavior (give ≈ 1 sen- tence justification why or why not)?
For a real gas obeying van der Waals equation CP-CV is a)R b)zero c) > R d)< R
4) Why does the relation Cp > Cv always hold for a gas? Can Cp < Cv be valid for a liquid?
If the heat capacities, Cv and Cp, for He are determined to be 18.708 J*K^-1 and 31.179J*K^-1, respectively, how many moles of gas are present? Assume the gas behaves ideally. Calculate the constant, y, used in calculations involving ideal gas adiabats using this data.
a. Given that the energy of an ideal gas is a function of temperature only, show how the conclusion can be reached that the enthalpy of an ideal gas is also only a function of temperature. b. Show that for an ideal gas Cp-Cv=R Hint: How much more heat is required to raise the temperature of the gas by 1K if the process is carried out at constant pressure rather than constant volume? Explain.
Derive how you can get Cp=KR/K-1 and Cv=R/K-1 from Cp/Cv = K