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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. 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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