The molar heat capacity of water in equilibrium with ice at constant pressure equals __________ Kcal/kg mole·°K___________________?
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Answer: B. ∞
Explanation
At the phase equilibrium melting point of ice, supplying heat results in a phase change at constant temperature, making the effective molar heat capacity approach infinity. Molar heat capacity is mathematically defined as the infinitesimal heat added divided by the corresponding temperature change of the system. Since melting ice absorbs latent heat without experiencing any temperature change, the denominator approaches zero, driving heat capacity toward infinity. Heat capacity measures the amount of thermal energy required to raise the temperature of a given substance by one degree. Phase transitions involve latent heat exchange, meaning added thermal energy breaks intermolecular bonds instead of increasing kinetic energy. Thermodynamic equilibrium between solid ice and liquid water occurs at standard melting point conditions under constant atmospheric pressure.
A heat capacity of zero would imply that adding thermal energy produces an infinitely large temperature change instantly. Finite numerical values like fifty or one hundred incorrectly assume that temperature must rise whenever heat enters the system. Constant temperature phase changes strictly defy finite heat capacity definitions because the temperature differential remains precisely at zero.
- Subject
- Engineering
- Category
- Chemical Engineering
- Topic
- —
- Difficulty
- medium
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