Two moles of ideal he gas are contained at a pressure of 1 atm and a temperature of 300 k. 34166 j of heat are transferred to the gas, as a result of which the gas expands and does 1216 j of work against its surroundings. the process is reversible. (note: c = 1.5r) calculate the final temperature of the gas

Explanation:

The given data is as follows.

       n = 2 mol,         P = 1 atm,         T = 300 K

        Q = +34166 J,         W= -1216 J (work done against surrounding)

        =

Relation between internal energy, work and heat is as follows.

      Change in internal energy () = Q + W

                                   = [34166 + (-1216)] J

                                   = 32950 J

Also,  

                      =

                 32950 J =

                            1321.06 K + 300 K =    

                                        = 1621.06 K

Thus, we can conclude that the final temperature of the gas is 1621.06 K.

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