(Image included with problem)
9.186E-1 moles of an ideal diatomic gas undergoes a transition from a to c along the diagonal path in the figure. The temperature of the gas at point a is 1310 K. During the transition, what is the change in internal energy of the gas? How much heat is added to the gas in going directly from a to c? How much heat must be added to the gas if it goes from a to c along the indirect path abc?
Without the figure....
To determine the change in internal energy of the gas, we need to use the first law of thermodynamics, which states that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system.
In this case, we are given the amount of moles of the gas (9.186E-1 moles) and the temperature at point a (1310 K). However, we need additional information to calculate the change in internal energy, such as the pressure or volume of the gas at points a and c.
Similarly, to determine the amount of heat added to the gas in going directly from a to c, we need information about the pressure or volume at those points.
Lastly, to calculate the amount of heat required to go from a to c along the indirect path abc, we need information about the pressure or volume at all three points.
Therefore, without the necessary information about the pressure or volume at the given points, we cannot calculate the change in internal energy or the amount of heat added to the gas.