he following chemical equations describe the same chemi-cal reaction. How do the free energies of these two chemical equations compare?
I KNOW THE ANSWER IS B BUT EXPLAIN YOUR REASONING!
(1) 2 H2O (l) ---> 2 H2 (g) + O2(g)
(2) H2O (l) ---> H2 (g) + 1/2 O2(g)
(a) ∆G°1=∆G°2
(b) ∆G°1=2 ∆G°2
(c) 2 ∆G°1=∆G°2
(d) None of the above
For a reaction
Go = -nFEo
Where n is the number of moles of electrons involved , F is the faraday's constant and Eo = Potential
In reaction 1, Number of moles of electrons involved are 4
as : Oxidation state of H changes from +1 to o and that of Oxygen from -2 to 0
Here two moles of H2O are involved. So number of electrons exchanged = 4
So, Go1 = -4FE0
Similarly in second reaction,
Number of moles of electrons involved = 2
So, G02 = -2FEo = -4FE0 /2 = Go1 /2
Go1 = 2Go2
Option B
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