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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?
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?
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.
Show that MSE(%) MSE0%rs) if R > 1 CV (x) 2 CV(y) Show that MSE(%) MSE0%rs) if R > 1 CV (x) 2 CV(y)
What is the heat capacity at constant volume, Cv, of an ideal gas, in ??? ?? °? if the constant pressure heat capacity, Cp = 0.124 ?? ??? ? and the molar mass of the material is 28 ton/ton-mole?
Extra Credit #5. that 45 = Cp In T2 - R ln P Show for an ideal gas That is changing temp, and pressure. Hints. Start with d H= Tas trap 1. Rearrange this so ds is alone on left side a. Recall that dH Cp dT . For ideal gas Cp is independent of T. 3. Use ideal gas law to eliminate v 4. Integrate. Write neatly and show every step.