Here I have another problem:
Calculate the melting point of ice under a pressure of 50 bar given that the melting point at 1 bar is 0°C. Assume that the density of ice under these conditions is 0.92 g/mL and the density of liquid water is 1.00 g/mL. The molar enthalpy of fusion of water is 6.01 kJ/mol.
dp/dT=ΔH/TΔV and they say that dp/dT=Δp/ΔT.
How can they say this?Afterwards, Δp/ΔT=ΔH/TΔV. Then:
ΔT=Δp·ΔV·T/ΔHNow Δp=4 900 000 Pa, ΔH=6010 J/mol and ΔV=18/1-18/0.92=-1.565·10
-3 dm
3/mol.
When plugging into the equation: ΔT=-348.34 K which is nonsense. What did I do wrong
?