what is the free energy change in kJ for the reaction below?
2NO3-(aq)+8H+(aq)+3Hg(l) <-->2NO(g)+4H2O(l)+3Hg2+(aq)
E0=0.106V
To calculate the free energy change (ΔG) for a reaction, you can use the equation:
ΔG = -nFΔE
Where:
- ΔG represents the free energy change
- n is the number of moles of electrons transferred in the balanced equation
- F is the Faraday's constant (96,485 C/mol)
- ΔE is the standard cell potential (E°) of the reaction
In this case, the balanced equation shows n = 6 (from the 6 electrons transferred when 3 Hg metal atoms are oxidized to Hg2+ ions).
The standard cell potential (E°) given is 0.106V.
Now, we can substitute these values into the equation:
ΔG = -nFΔE
ΔG = -(6 mol)(96,485 C/mol)(0.106 V)
By performing this calculation, you can find the value of ΔG in joules. To convert it to kilojoules, you can divide the result by 1000:
ΔG = -(6)(96,485)(0.106) J = -61,352.26 J
Therefore, the free energy change (ΔG) for the reaction is approximately -61,352.26 J.