I would really appreciate it if someone could give me the answers to this proble

Question

I would really appreciate it if someone could give me the answers to this problem (typed preferably), as well as somewhat of an explanation to how... Thanks

A 3.15mol sample of an ideal diatomic gas expands adiabatically from a volume of 0.1550m3 to 0.745m3 . Initially the pressure was 1.00 atm.

Part A

Determine the initial and final temperatures.

Enter your answers numerically separated by a comma.

Part B

Determine the change in internal energy.

Part C

Determine the heat lost by the gas.

_______

Part D

Determine the work done on the gas. (Assume no molecular vibration.)

Explanation / Answer

Let the inital volume be V1

apply PV= nRT at initial conditions

T1 = P1 V1 / nR

T1 = 1 x 0.155 x 1000 / 3.15 x 0.0821

T1 = 599.346 K

Given adiabatic process

for diatomic gas

gamma Y = 1.4

TV^(Y-1) = constant

so

T1 V1 ( 1.4 -1) = T2 V2 ( 1.4-1)

T2 = T1 ( V1 / V2 ) ^ 0.4

T2 = 599.346 ( 0.155/0.745) ^ 0.4

T2 = 319.85 K

now apply PV = nRT at final conditions

P = 3.15 x 0.0821 x 319.85 / 0.745 x 1000

P = 0.111 atm

Work done = ( P1V1 -P2V2 ) / ( Y-1)

Work done = ( 1 x 0.155 x 1000 - 0.111 x 0.745 x 1000) / ( 1.4 -1)

Work done = 180.7625 J

in adiabatic procees

Heat lost = 0

SO change in internal energy = - work done

Change in internal energy = - 180.7625 J

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