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.

answer is: c. the experiment shows that the red substance experienced a chemical change.

this is chemical change (chemical reaction), because two new substances are formed (metalig liquid and gas), the atoms are rearranged and the reaction is followed by an energy change.

this is example of chemical decomposition.

chemical decomposition (analysis) is the separation of a single chemical compound into its two or more elemental parts or to simpler compounds.  

chemical decomposition is opposite of chemical synthesis.

what is the question?