Check all the correct statements. The internal energy of an ideal gas (those tha
ID: 1871370 • Letter: C
Question
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. U= qv only for a monoatomic ideal gasExplanation / Answer
1. Correct. For an ideal gas internal energy is a function of temperature.
2. Incorrect. For any gas internal energy is function of pressure, volume and number of molecules also.
3. False, because heat capacity depends on number of moles of ideal gas which in turn depends on mass of constituent molecules.
4. Correct. At constant temperature internal energy increases with decrease of volume and volume decreases with increase of pressure.
5. False.
6. Correct. For a cyclic process internal energy is constant or change in internal energy is zero.
7. True. When process takes place with no change of temperature internal energy remains same or change in internal energy is zero.
8. False.