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Grade: 11

                        

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.

4 years ago

Answers : (1)

navneet
34 Points
							
Since heat is absorbed here at constant pressure so ΔH = 1440 calories
ΔU can be calculated by using the formula :ΔU=ΔH-PΔV
P= 1atm, ΔV = 0.0196L - 0.180L = 0.0016 L
PΔV = 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
 
4 years ago
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