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 • 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.
FREE Expert 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).
Problem Details
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.
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Heat Capacity concept. You can view video lessons to learn Heat Capacity. Or if you need more Heat Capacity practice, you can also practice Heat Capacity practice problems.
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Based on our data, we think this problem is relevant for Professor Berns' class at NU.
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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.