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posted by  JDINH412 on 5/13/2008 3:34:03 AM  |  status: Live  

Work in Thermodynamic Process

Course Textbook Chapter Problem
General Physics College Physics (7th) by Serway, Faughn, Bennett 12 55
Question Details:
One mole of neon gas is heated from 308 K to 417 K at constant pressure.
 
(a) Calculate the energy Q transferred to the gas in Joules
(b) Calculate the change in the internal energy of the gas in Joules
(c) Calculate the work done on the gas. Note that neon has a molar specific heat of c = 20.79 J/mol·K for a constant pressure process in Joules
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posted by richmondMike on 5/13/2008 3:55:21 AM  |  status: Live
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JDINH412's comment:
"thank you very much for your help!"
Response Details:
Given the number of  mole of the neon gas is n = 1mol, T1 = 308K, and T2 = 417K.
(a) Under constant pressure, the energy transferred to the gas is dQ = nCPdT = (1mol)(20.79J/mol-K)(417K - 308K) = 2266.11J ˜ 2270J.
(b) CV = CP - R = 20.79J/mol-K - 8.31J/mol-K = 12.48J/mol-K
The change in the internal energy of the gas is dU = nCVdT = (1mol)(12.48J/mol-K)(417K - 308K) = 1360J.
(c) The work done by the gas is dW = dQ - dW = 2270J - 1360J = 910J.
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