Calculate the work done (in joules) when 1.0 mole of water...

Calculate the work done (in joules) when 1.0 mole of water is frozen at $0^{\circ} \mathrm{C}$ and 1.0 atm. The volumes of one mole of water and ice at $0^{\circ} \mathrm{C}$ are $0.0180 \mathrm{L}$ and $0.0196 \mathrm{L},$ respectively.

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Key Concepts

Pressure-Volume Work

In thermodynamics, work can be performed by or on a system when there is a change in its volume under an applied pressure. This type of work, often denoted as pressure-volume work, is commonly calculated using the expression W = -p?V, where p represents the constant pressure and ?V is the change in volume of the system. The sign indicates whether work is done on the system or by it, following the conventional thermodynamic sign convention.

Constant Pressure Process

A constant pressure process is one where the external pressure remains unchanged during the transformation. In such processes, the work associated with a volume change can be simply computed using the pressure-volume work formula. This concept is central to many practical scenarios in chemistry and physics, including phase transitions, where a substance may expand or contract without a change in external pressure.

Unit Conversion in Thermodynamics

Thermodynamic calculations often require the conversion of units to ensure consistency and accuracy. For instance, pressure-volume work calculated in units such as atmospheres and liters must be converted into joules using the appropriate conversion factor (1 atm·L equals approximately 101.325 joules). This conversion is crucial when interrelating macroscopic energy changes with the standard SI unit of energy.

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