A cylinder with a movable piston contains 3.00 mol of N2 gas (assumed to behave 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.

Solution 25E Problem (a) To calculate change in Temperature dT at constant Volume Step 1: No of moles n = 3 Heat added to the system Q = 1557 J Gas Constant R = 8.314 J/mol.K Volume is constant