A mixture initially contains A, B, and C in the following concentrations: [A] = 0.600 M , [B] = 1.30 M , and [C] = 0.500 M . The following reaction occurs and equilibrium is established: A+2B⇌C At equilibrium, [A] = 0.410 M and [C] = 0.690 M . Calculate the value of the equilibrium constant, Kc.

Explanation:

Chemical equation for the given reaction is as follows.

Initial :    0.6       1.30           0.5

Final :   (0.6 - x)  (1.30 - 2x)  (0.5 + x)

It is given that at equilibrium, [A] = 0.410 M.

So,    x = (0.600 - 0.410)

           = 0.19 M

Hence, [B] will also be calculated as follows.

       [B] =

             = 0.92

Now, we will calculate the value of equilibrium constant as follows.

                  =      

                  =

                  = 1.988

Thus, we can conclude that the value of the equilibrium constant, is 1.988.

the enthalpy of formation of water is given as -285.8kj/mol, which states that the enthalpy of formation is negative.

negative enthalpy of formation indicates that the heat is released during the reaction process. the heat is released from reaction to the surroundings the enthalpy is expressed with a negative sign with the energy given out in the reaction process.

the formation of water takes place by giving out heat which is -285.8 kj/mol.