Chemical Engineering - Stoichiometry - Discussion

The molar heat capacity of water in equilibrium with ice at constant pressure is commonly referred to as the heat capacity of ice. It represents the amount of heat energy required to raise the temperature of one mole of ice by 1 degree Celsius at constant pressure.

For ice near its melting point, this heat capacity is approximately 37.7 J/ (mol·K). It's important to note that this value can vary slightly with temperature, but it's commonly considered near 0 degrees Celsius.

Water, in equilibrium with ice has a steady temperature of zero degree Celsius.

Water, in the liquid state, has a specific heat of exactly 1 calorie per gram.

Molar mass of water is 15.999 + 2.016 = 18.015 grams per mole.

Therefore, molar heat capacity of water at zero degree Celsius is

=18.015*1 Calorie/mole/K
=18.015*1*4.184 Joules/mole/K.
=75.4 J/mole/K.

Heat capacity at constant pressure may be defined as the rate of change of enthalpy with temperature at constant pressure.

Cp=dH/dT. Since water and ice is at equilibrium, there is no change in temperature. They are at same temperature.

So dT =0 and we know that something divided by 0 is infinity. Thus Cp= infinity ( at constant pressure).

Molar heat capacity is the amount of heat required to increase 1 mole of a substance by 1 degree.

At Water-ice equilibrium, the temperature remains 0 C. So no matter what ever amount of heat you add, its temperature remains 0 C theoretically.

1&0 is correct answer.