Solution: Consider a balloon filled with helium at the following conditions.313 g He 1.00 atm 1910. L Molar Heat Capacity = 20.8 J/°C • molThe temperature of this balloon is decreased by 41.6°C as the volume decreases to 1643 L, with the pressure remaining constant. Determine q, w, and ΔE (in kJ) for the compression of the balloon.

Solution: Consider a balloon filled with helium at the following conditions.313 g He 1.00 atm 1910. L Molar Heat Capacity = 20.8 J/°C • molThe temperature of this balloon is decreased by 41.6°C as the volume de

Problem

Consider a balloon filled with helium at the following conditions.

313 g He 

1.00 atm 

1910. L 

Molar Heat Capacity = 20.8 J/°C • mol

The temperature of this balloon is decreased by 41.6°C as the volume decreases to 1643 L, with the pressure remaining constant. Determine q, w, and ΔE (in kJ) for the compression of the balloon.

Solution

Recall: The change in internal energy (ΔE or ΔU) is given by:

The formula for work at constant pressure is:

where ΔV = change in volume (final V – initial V).

The formula for heat at constant pressure is:

where n = moles of compound, Cp = molar heat capacity at constant pressure, and ΔT = change in temperature (final T – initial T).

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