You have 1.7 moles of a fictitious ideal gas whose molar specific heat values ar

Question

You have 1.7 moles of a fictitious ideal gas whose molar specific heat values are C_v = 17.89 J/mol middot K) and C_p = 26.20 J/(mol middot K). The gas expands from an initial volume of 0.0194 m^3 to a final volume of 0.0363 m^3 at a constant pressure of 2.07 atm. What was the initial temperature? K (Do not enter units) What is the final temperature? K (Do not enter units) How much work is done by the gas? How much thermal energy (heat) flows into the gas? What is the change in the internal energy of the gas?

Explanation / Answer

by ideal gas law

PV = nRT

T = PV/nR

R = 8.2 x 10^-5 m^3 atm K^-1 mol^-1

P = 2.07 atm

n = 1.7

V = 0.0194 m^3

T = 288

part b )

at constant pressure

V1/T1 = V2/T2

0.0194/288 = 0.0363/T2

T2 = 538.89

part c )

W = P*dV

P = 2.07 atm = 2.07 x 1.013 x 10^5 Pa

dV = (0.0363 - 0.0194)

W = 3543.78 J

part d )

thermal energy = n*Cp*dT

Q = 11174.64 J

part e )

dU = nCv*dT

dU = 7630.32 J

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