Question
Asked Nov 10, 2019
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4.00 L of ar and 2.50 L of he, each at 298 K and 1.50 atm, were mixed isothermally and isobarically. The mixture was then expanded to a final volume of 20.0 L at 298 K. Write chemical processes for each step, and determine the change in entropy for the complete process.

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Expert Answer

Step 1

Calculation of number of moles :

Ideal Gas Equation:

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PV=nRT PV n= RT Argon: 4L 1.5atm n (0.08206L.atm/K.mol) 298K n 2.453mol Heliun 2.5L 1.5atm n (0.08206L.atm/K.mol) 298 n 0.1533mol

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Step 2

Calculation of mole fraction:

Mole fraction two component system,

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n x= Argon 0.2453 mol 0.2453mol+0.1533 mol 0.2453mol 0.3986mol -0.6154mol 0.1533mol 0.2453mol+0.1533mol 0.1533 0.3986 0.3846mol

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Step 3

Entropy of mixing o...

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--R{14 Inx +ng, Inx) -(8.314J/mol.K)(0.2453mol)In(0.6514)+(0.1533mol)In(0.3846)) -(8.314J/molK)(-0.2656 mol) 2.2081 J/K

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