?U = 0 for any process that does not result in a change in temperature.
A cyclic path (initial state = final state) always results in ?U = 0
?U= qv only for a monoatomic ideal gas
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)
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 CO2 is greater than the heat capacity of He because CO2 is more polar.
Check all the correct statements. AU-0 for any process that does not result in a change in temperature. A cyclic path (initial state-final state) always results in AU-0 ÎU- Io only for a monoatomic ideal gas 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) 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 CO2 is greater than the heat capacity of He because CO2 is more polar. Submit My Answers Give Up Incorrect; Try Again; 2 attempts remaining
