Question

At the normal melting point of H2O, ?_fus H_m = 6010 J mol-1. Calculate the melting point for ice at 2300 bar if both ?_fus H_m and densities ?(s)= 917 kg m-3 and ?(l)= 997 kg m-3 assumed constant.

Answer #1

The normal melting point of H2O is 273.15 K, and Hfusion= 6010
J mol–1. Calculate the decrease in the normal freezing point at 100
and 500 bar assuming that the density of the liquid and solid
phases remains constant at 997 and 917 kg m–3, respectively.

1. At the normal melting point of ice
∆Hfus= 6.007 kJ mol−1 and
∆Sfus= 22.00 J K−1
mol−1.
a) What is ∆Gfusat the normal melting
point? Look at your answer. Is it correct? Why or why not?
b) Determine ∆G for freezing water at 1 atm and
-10oC assuming that
∆Hfusand
∆Sfusdo not change much over the 0 →
−10oC temperature range.
c) Determine ∆G for freezing water at 1 atm and
-10oC assuming that
∆Hfusdoes not change much over...

The normal melting point of substance A is 320C. Melting
heat is a function of temperature. Determine the melting
temperature of substance A at 10 bar.
Data :
Density of liquid A = 10200
kg/m3
Density of Solid A = 12000 kg/m3
For liquid A CpL =
30,0-3,1 x 10-3T (J/mol.K)
For solid A CpS = 20,0 +
9x10-3T (J/mol.K)
Tref =
320oC
ΔHreferime = 4900
J/mol
MA = 250 kg/kmol

The normal freezing point of water is 0.0 oC. At this temperature
the density of liquid water is 1.000 g/ml and the density of ice is
0.917 g /ml. The increase in enthalpy for the melting of ice at
this temperature is 6010 J/mol. What is the freezing point of water
at 200 atmospheres?

he normal freezing point of water is 0.0 degrees celsius. at
this temperature the density of liquid water is 1.000 g/mL and
density of ice is 0.917 g/mL. the increase in enthalpy for the
melting ice at this temperature is 6010 J/mol. What is the freezing
point of the water at 200 atms?

For mercury, ∆Hfuso = 2.292 kJ
mol-1, and its normal freezing point is 234.3 K. The
change in molar volume on melting ∆Vfus = 0.517
cm3 mol-1. Calculate the melting point of
mercury at 20.0 bar.

Gold has an equilibrium melting temperature of 1337 K at 1 atm
and an enthalpy of fusion of 12,550 J/mol. Find the pressure at
which the equilibrium melting temperature is 1400 K.
Using this answer, calculate the entropy change for melting 1 mol
of gold. The densities of solid gold and liquid gold are 19.3 g/mL
and 17.3 g/mL and are assumed to be approximately constant under
all conditions

Assume that the density of solid water is 920 kg m-3 and that of
liquid water is 1000 kg m-3. Calculate the change of the melting
temperature, T, of ice for the process of changing pressure from
100 kPa to 1850 kPa. Use fusH = 6010 J mol-1 for water.

Quantity
per gram
per mole
Enthalpy of fusion
333.6 J/g
6010. J/mol
Enthalpy of vaporization
2257 J/g
40660 J/mol
Specific heat of solid
H2O (ice)
2.087 J/(g·°C) *
37.60 J/(mol·°C) *
Specific heat of liquid
H2O (water)
4.184 J/(g·°C) *
75.37 J/(mol·°C) *
Specific heat of gaseous
H2O (steam)
2.000 J/(g·°C) *
36.03 J/(mol·°C) *
At 1 atm, how much energy is required to heat 49.0 g of H2O(s)
at − 18.0 °C to H2O(g) at 135.0 °C? Heat transfer...

Trouton’s rule states that the entropy of boiling at the normal
point is 85 J/mol * K. (a) Does the data from Example 3.2 support
Trouton’s rule? (b) H2O has a heat of vaporization of 40.7 kJ/mol.
Does the Delta vapS for H2O at its normal boiling point support
Trouton’s rule? Can you explain any deviation? (c) Predict the
boiling point of cyclohexane, C6H12, if its Delta vapH is 30.1
kJ/mol. Compare your answer to the measured normal boiling point...

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