(adsbygoogle = window.adsbygoogle || []).push({}); 1. The problem statement, all variables and given/known data

For both H20 and D20:

Cp = 75.5 J/mole-k for the liquid Cp = 37.8 J/mole-k for the solid ΔHfus=6.01 kJ/mole.

Liquid H20 and D20 form an ideal solution.

a) One mole of liquid H20 at 10 C is mixed with four moles of LIQUID D20 at 0 C in an insulated container.

Determine ΔS.

b) One mole of liquid H20 at 10 C is mixed with four moles of SOLID D20 at 0 C in an insulated container.

Determine ΔS.

2. Relevant equations

ΔSmixing = -R(nX1lnX1 + nX2lnX2)

3. The attempt at a solution

I found

ΔSmixing = -R(nX1lnX1 + nX2lnX2) = -8.324[(1mol)(1/5)ln(1/5) + (4mol)(4/5)ln(4/5)] = 8.612 j/mol-k

I don't really understand the question. Can someone explain some of he concepts I need to know or direct me to somewhere where it sums it up?

What are the steps to solving this? What do I have to think about? (Like...I know X, so I get Y because of Z)

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# Homework Help: Determine ΔS when mixing

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