Question

1. At the normal melting point of ice
∆*H** _{fus}*= 6.007 kJ mol

a) What is ∆

b) Determine ∆*G* for freezing water at 1 atm and
-10^{o}C assuming that
∆*H** _{fus}*and
∆

c) Determine ∆*G* for freezing water at 1 atm and
-10^{o}C assuming that
∆*H** _{fus}*does not change much over the 0 →
−10

Answer #1

a)

Melting point of ice is T= 273.15K

So

The answer is wrong as should be zero at 273.15K as at that temperature there is an equilibrium between ice and water.

b) At T=273.15-10=263.15K ,

c) Entropy change is given by .

so if the molar specific heat at constant pressure c_{p}
is given then we can find the
and thus find
as done in part b.

The normal melting point of H2O is 273.15 K, and Hfusion= 6010
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phases remains constant at 997 and 917 kg m–3, respectively.

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.

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.

What amount of thermal energy (in kJ) is required to convert 220
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melting point of water is 0 °C and its normal boiling point is 100
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vaporization of water at its normal boiling point is 40.7 kJ mol-1
The specific heat capacity of ice is 2.09 J g-1 °C-1 The specific
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What amount of thermal energy (in kJ) is required to convert 216
g of ice at -30 °C completely to water vapour at 198 °C? The
melting point of water is 0 °C and its normal boiling point is 100
°C. The heat of fusion of water is 6.02 kJ mol-1 The heat of
vaporization of water at its normal boiling point is 40.7 kJ mol-1
The specific heat capacity of ice is 2.09 J g-1 °C-1 The specific
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For cobalt, Co, the heat of
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15.5 kJ/mol.
The entropy change when 1.70 moles of liquid
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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
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A and B. Calculate ΔSsurr and ΔStotal at 1060 K .Express your
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he normal freezing point of water is 0.0 degrees celsius. at
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Constants
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heat capacity of Hg(l)
28.0 J/(mol·K)
melting point
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