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3 years ago

For a cell whose potential is –0.46 v with 3 moles of electrons exchanged, what is ΔG ? ΔG = –nFE°cell

Chemistry

2 answers:

jeka57 [31]3 years ago

8 0

Answer:

133kj

Explanation:

Nimfa-mama [501]3 years ago

4 0

ΔG is 133kJ

ΔG = –nFE°cell
ΔG = free energy of the reaction = ?
n = no of moles of electrons exchanged in the reaction = 3
F = Faraday's constant (9.648456 x $10^{4}$ C/mol) $E_{0}$ = cell potential = –0.46 v

⇒ ΔG = –nFE°cell
⇒ ΔG = - (3 mol)(9.648456 x $10^{4}$ C/mol) (-0.46 J/C) ⇒ ΔG = +133148 J ≈ 133 kJ

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Energy of one mole of photons = 6.02 × 10²³ × 6.63 × 10−³⁴ × 3 × 10⁸/5.20 × 10-⁷

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Where m is mass of substance, c is specific heat capacity, ΔT is temperature difference

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