please write the steps for these two questions. thanks 2.75 moles of an ideal ga

Question

please write the steps for these two questions. thanks

2.75 moles of an ideal gas is expanded from 375 K and an initial pressure of 4.75 bar to a final pressure of 1.00 bar, and Cp,m = 5R/2. Calculate the work (w) for the following two cases: a) The expansion is isothermal and reversible b) The expansion is adiabatic and reversible c) Without resorting to equations, explain why the result to part (b) is greater than or less than the result to part (a)

One mole of an ideal gas with Cv,m = 3R/2 initially at 325 K and 1.50x10 to the 5 Pa undergoes a reversible adiabatic compression. At the end of the process, the pressure is 2.50x10 to the 6 Pa. Calculate the final temperature of the gas. Calculate q, w, deltaU, and deltaH for this process.

Explanation / Answer

(a)

n = 2.75 mole

Pi = 4.75 bar

Pf = 1 bar

T = 375 K

work = nCp ln(Pi/Pf)

= 89.06 KJ

(b)

Cp = 5/2R, means it is monoatomic gas

so f = 3

thus gamma(y) = 1=2/f = 5/3

V = nRT/P = 1805

Adibatic work = PV^y(Pi^y - Pf^y)/(1-y)

= 1237.174 KJ

(c) adiabatic work is greater than part a because of slope of grpah, which is equal to 1 in part a and gamma(y) in case of b

and gamma = 5/3 >1

final temperature will be 541 K

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