The assignment: a fixed quantity of an ideal gas (r 0.28 kj/kgk; cv-0.71kj/kgk) is expanded from an initial condition of 35 bar, 500°c, 0.1m, to a final state of1.3mand 20c using a reversible polytropic process. calculate: (i) the index of expansion; (ii) the change in internal energy; (ii)the amount of heat transferred to or from the gas. show all your working clearly-and legibly if you're handwriting your submission.

Index of expansion: 4.93

Δu = -340.8 kJ/kg

q = 232.2 kJ/kg

Explanation:

The index of expansion is the relationship of pressures:

pi/pf

The ideal gas equation:

p1*v1/T1 = p2*v2/T2

p2 = p1*v1*T2/(T2*v2)

500 C = 773 K

20 C = 293 K

p2 = 35*0.1*773/(293*1.3) = 7.1 bar

The index of expansion then is 35/7.1 = 4.93

The variation of specific internal energy is:

Δu = Cv * Δt

Δu = 0.71 * (20 - 500) = -340.8 kJ/kg

The first law of thermodynamics

q = l + Δu

The work will be the expansion work

l = p2*v2 - p1*v1

35 bar = 3500000 Pa

7.1 bar = 710000 Pa

q = p2*v2 - p1*v1 + Δu

q = 710000*1.3 - 3500000*0.1 - 340800 = 232200 J/kg = 232.2 kJ/kg

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hey , the answer is c