1. The problem statement, all variables and given/known data n = 1.46 moles of ideal gas are heated isochorically (at constant volume) from tepmerature To = 649 oC to temperature Tf = 1184 oC. Find: a) Work done on the system. b) Change in Internal Energy of the system. c) The total heat, Q, added or removed from the system. 2. Relevant equations Change in I.E. = Q + W KE (avg) = T = 3/2kT, where k = 1.38 x 10^-26 kJ/K 3. The attempt at a solution a) Since this is an isochoric system, work done is ZERO! (No issues here.) b,c) Change in Internal Energy, therefore is equal to Q, by the first equation, Change in IE = Q + W. So, we can calculate change in IE, by change in KE. KE = (3/2kT) for a monatomic gas. so, change in KE = 3/2(k)(Tfinal - Tinitial), = (3/2)(1.38E-26)(1500 K - 704K) = change in IE = Q = 1.65 x 10^-23. Am I reading the problem incorrectly? Many thanks in advance once again!