3. How many moles in 28 grams of CO2?
2 answers:
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where, E^{o} (Ag+/Ag) = std. reduction potential of Ag+ = 0.7994 v
and Sn2+/Sn = std. reduction potential of Sn2+ = -0.14 v
Thus, E^{o}cell = 0.7994v - (-0.14v) = 0.9394 v
Now, ΔG^{o} = -nF
where, n = number of electrons = 2
F = Faraday's constant = 96500 C
∴ΔG^{o} = 2 X 96500 X 0.9394 = -1.18 X
Now, using Nernst's Equation we have,
E_{cell} = 0.9765 v
Finally, ΔG = -nFE = -2 X 96500 X 0.9765 = -1.88 X