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Calculate ΔS if 2.10 mol of liquid water is heated from 0.00 ∘C to 13.5 ∘C...

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Chemistry

Calculate ΔS if 2.10 mol of liquid water is heated from 0.00 ∘Cto 13.5 ∘C under constant pressure if CP,m=75.3J⋅K−1⋅mol−1.

The answer the the problem above is 7.62 J/K

The melting point of water at the pressure of interest is 0.00∘C, and the enthalpy of fusion is 6.010 kJ⋅mol−1. The boiling pointis 100. ∘C, and the enthalpy of vaporization is 40.65 kJ⋅mol−1.Calculate ΔS for the transformation of the same amount ofwater

H2O(s,0.00∘C) →H2O(g,100.∘C)

Can you help me solve the second question?

Answer & Explanation Solved by verified expert
3.6 Ratings (616 Votes)
There are 3 processes in H2O s 000 oCH2O g 100 oCProcess 1 Conversion of solid water to liquid water at 000oCS1 n Hfus Twheren moles of water 210 molHfus enthalpy of fusion at melting    See Answer
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