Answer:
If an ideal gas does positive work on its surroundings, we can assume that the gas has undergone a decrease in its internal energy. This is based on the first law of thermodynamics, which states that the change in the internal energy of a system is equal to the heat added to the system minus the work done by the system.
When an ideal gas does positive work on its surroundings, it means that the gas has transferred energy to the surroundings by performing work. This results in a decrease in the internal energy of the gas because it has lost some of its energy to the surroundings.
Therefore, we can assume that the temperature of the gas has decreased because the internal energy of the gas is proportional to its temperature. This assumption is based on the ideal gas law, which states that the pressure, volume, and temperature of an ideal gas are related. If the pressure and volume of the gas remain constant, a decrease in the temperature of the gas will result in a decrease in its internal energy.
In summary, if an ideal gas does positive work on its surroundings, we can assume that the gas has undergone a decrease in its internal energy and its temperature has decreased.
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