Check all the correct statements. The internal energy of an ideal gas (those that obey PV...

Check all the correct statements.

The internal energy of an ideal gas (those that obey PV = nRT) depends only the temperature of the system.

The internal energy of any gas depends only the temperature of the system.

The heat capacity of an ideal gas does not depend on what molecules the gas is made of.

At constant temperature, the internal energy of a real gas increases with increasing pressure because molecules are closer together. We assume that the conditions are such that attractions dominate over repulsions (i.e. the pressure values are not too high)

At constant temperature, the internal energy of a real gas decreases with increasing pressure because molecules are closer together. We assume that the conditions are such that attractions dominate over repulsions (i.e. the pressure values are not too high)

A cyclic path (initial state = final state) always results in ∆U = 0

∆U = 0 for any process that does not result in a change in temperature.

ΔU= qv only for a monoatomic ideal gas

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genius_generous answered 1 year ago

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