Selena notes that CP is greater than CV, and asks Herbert to explain why. Which explanation is correct?\ "For a thermodynamic process in an ideal gas at constant volume, the work done is zero. Therefore, all heat supplied is used in increasing the temperature. At constant pressure, some of the heat supplied is used by the system in doing work. This means that more heat is needed to increase the temperature by a given amount, which implies CP < CV"\ "For a thermodynamic process in an ideal gas at constant volume, the work done is zero. Therefore, all heat supplied is used in increasing the temperature. At constant pressure, all of the heat supplied is used by the system in doing work. This means that more heat is needed to increase the temperature by a given amount, which implies CP > CV." \ "For a thermodynamic process in an ideal gas at constant pressure, the work done is zero. Therefore, all heat supplied is used in increasing the temperature. At constant volume, some of the heat supplied is used by the system in doing work. This means that more heat is needed to increase the temperature by a given amount, which implies CP > CV."\ "For a thermodynamic process in an ideal gas at constant volume, the work done is zero. Therefore, all heat supplied is used in increasing the temperature. At constant pressure, some of the heat supplied is used by the system in doing work. This means that more heat is needed at constant pressure to increase the temperature by a given amount, which implies CP > CV."