Question: A cylinder with a movable piston contains 3.00 mol of N2 gas (assumed to he have like an ideal gas). (a) The N2 is heated

A cylinder with a movable piston contains 3.00 mol of N2 gas (assumed to he have like an ideal gas).
(a) The N2 is heated at constant volume until 1557 J of heat have been added. Calculate the change in temperature.
(b) Suppose the same amount of heat is added to the N2, but this time the gas is allowed to expand while remaining at constant pressure. Calculate the temperature change.
(c) In which case, (a) or (b), is the final internal energy of the N2 higher? How do you know? What accounts for the difference between the two cases?

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