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The molar volumes of ice and water are 0.0196 and 0.0190 litres per mole at 273K. If ΔHefor the transition of ice to water is 1440 calories per mole at 1 atm pressure, find ΔU.
Since heat is absorbed here at constant pressure so ΔH = 1440 caloriesΔU can be calculated by using the formula :ΔU=ΔH-PΔVP= 1atm, ΔV = 0.0196L - 0.180L = 0.0016 LPΔV = 1*0.0016= 0.0016Latm = 0.0016*24.217calories. (1Latm =24.217 calories)So ΔU = 1440 cal-0.0016*24.217cal≈1439.96 calories .There is negligible work done here.so you can write ΔH≈ΔU
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