For the reaction a(g) + 2 b(g) ↔ c(g) the initial partial pressures of gases a, b, and c are all 0.109 atm. once equilibrium has been established, it is found that pc = 0.047 atm. what is δg° for this reaction (in kj/mol) at 25°c?

Explanation:

As the given reaction is as follows.

The given data is as follows.

Initially,     = 0.109 atm,      = 0.109 atm,

                = 0.109 atm

And, at equilibrium

        = 0.047 atm

Therefore, change in will be calculated as follows.

                    0.109 - 0.047

                 = 0.062 atm

Hence, = (0.109 + 0.062) atm = 0.171 atm

= atm

                        = 0.233 atm

Now, calculate the value of as follows.

                    =

                    = 5.06

Also, we known that

Hence, calculate the value of as follows.

                      =

                       =

                      = -4017.05 J/mol

or,                   = -4.017 kJ/mol              (as 1 kJ = 1000 J)

Thus, we can conclude that the value of for the given reaction is -4.017 kJ/mol.

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.