Which molecules will move faster?

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The discussion revolves around the Kinetic Molecular Theory (KMT) and its application to two balloons filled with helium gas at different volumes. The key question is whether the gas molecules in the 5-liter balloon move faster than those in the 10-liter balloon, assuming constant temperature. It is argued that according to KMT, the speed of gas molecules is determined solely by temperature, suggesting both balloons should have molecules moving at the same speed. However, a conflict arises with Gay-Lussac's law, which indicates that an increase in volume correlates with an increase in temperature, potentially leading to faster-moving molecules in the larger balloon. This creates confusion regarding the relationship between volume, temperature, and molecular speed in gases.
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In class today, we were talking about the Kinetic Molecular Theory and the combined gas law. I was understanding everything until our teacher threw in a question that confused me really bad

Suppose we fill two balloons with Helium gas. One of them is filled 5 liters of He and the other to 10 Liters. The molecules of which balloon will move faster?

He didn't mention anything about the temperature, so I'm assuming constant temperature here because inflating balloons doesn't change temperature. Nevertheless, this question has my head spinning; a detailed explanation would be appreciated
 
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Well I postulated that the molecules in both balloons would move at the same speed; this is because according to the KMT, Kinetic Energy of gas particles is dependent only on temperature, so they should be at the same speed. But because of Gay-lussac's law, Volume is directly proportional to temperature, so if the volume increases, the temperature should increase and thus make the molecules within the 10 L faster. But this contradicts the KMT since it states that KE of these molecules is dependent ONLY on temperature
 
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