From the calorimetric data, calculate δh for the reaction that occurs on mixing. assume that the calorimeter absorbs only a negligible quantity of heat, that the total volume of the solution is 100.0 ml, and that the specific heat and density of the solution after mixing are the same as that of pure water.

Explanation:

It is assumed that concentration of given is 1.0 M and its volume is 50.0 ml or L (as 1 L = 1000 mL).

For KOH, concentration is 2.00 M and volume is 50.0 ml or L.

= and =

Therefore, the given reaction equation will be as follows.

Hence, calculate the moles of copper sulfate as follows.

            Moles of

                                =

                                = 0.05 mol

Also, the number of moles of KOH will be as follows.

           Moles of KOH = (molarity) × (volume)

                                     =

                                     = 0.10 mol

Therefore, moles formed = moles consumed

                  0.5 × (moles of KOH consumed)

                = 0.05 mol

It is given that volume of solution = 100.0 mL

Hence, mass of solution = (Volume of solution) × (density of solution)

                                        = (100.0 mL) × (1.00 g/mL)

                                         = 100.0 g

Also, heat absorbed by solution will be as follows.

             q =

                 =

                 = 2594.08 J

So, heat lost by reaction = -(Heat absorbed by solution)

As, heat lost by reaction = -(2594.08 J)

therefore, heat absorbed by reaction = 2594.08 J

Now, calculate the change in enthalpy as follows.

                           =

                            = -51881.6 J/mol

or,                        = -51.9 kJ/mol              (as 1 kJ = 1000 J)

Thus, we can conclude that for the given reaction that occurs on mixing is -51.9 kJ/mol.      

while cooking a piece of 1/2 pound beef steak, a cast iron pan (2.4kg in weight) was heated 260 celsius.