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using standard electrode potentials, calculate δg∘ and use its value to estimate the equilibrium constant for each of the reactions at 25 ∘c. part a pb2 (aq) mg(s)→pb(s) mg2 (aq)

Respuesta :

The equilibrium constant can be obtained using ΔG°rxn = -RT lnK.

On the basis of this, 2H+ + 2e- → H2(g) reduction.

Therefore E° = 0V

Pb2+ + 2e- ⇄ Pb(s) - 0.126

Mg2+ + 2e- ⇄ Mg(s) -2.372

For total E°cell potential,

E°cell = Ered - Eoxd

Eoxd = -Ered of the one being oxidised

E°cell = -2.372 - (-0.126) = -2.246

E°cell = -2.246 V

Thus, calculating dG:

dG = -n x F x E°cell

dG = -2*96500*(-2.246)

=433478 J/mol

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