Use the standard enthaplies of formation to calculate the standard change in enthaply for the melting of ice. (-291.8 kj/mol for h20 (s). use this value to calculate the mass of ice required to cool 355 ml of a beverage from the room temperature (25 degree celsius) to 0 degree celsius. assume that the specfic heat capacity and the density of the beverage are the same as those of water.

Explanation:

The given reaction is as follows.

Hence, using standard values heat of fusion will be calculated as follows.

                  = -285.8 kJ/mol - (-291.8 kJ/mol)

                  = 6 kJ/mol

Therefore, heat released from beverage will be calculated as follows.

           q =

               =

               = -37133 J

or,           = -37.133 kJ         (as 1 J = 0.001 kJ)

Now, heat gained by ice = - heat released by the beverage

                                         = - (-37.133 kJ)

                                         = 37.133 kJ

Therefore, calculate the mass of ice as follows.

          Mass of ice =

                              = 111.40 g

Thus, we can conclude that mass of ice is 111.40 g.        

the right answer is c i just did the question.