Calculate the E_cell degree and delta G degree for the Cu^+2/Cu and Al^+3/Al half-cells. Is this half-cell reaction spontaneous under standard conditions? Al^3+(aq) + 3 e^- rightarrow Al (s) E degree = -1.66 V Cu^2+(aq) + 2 e^- rightarrow Cu(s) E degree = + 0.34 V E_cell degree = + 2.00 V: delta G degree = – 1158 kJ or -1.158 kJ or -1.158 times 10^6 J: since delta G degree negative the reaction will occurs spontaneously under standard conditions.
Calculate the Ecell and delta G for the cu2+/cu and Al+32/Al half cells
E˚cell = E˚cathode – E˚anode
E˚cell = 0.34 v – (-1.66 v) = +2.00 v——————-ANSWER
= (-6 mol e–)(96458 C/mol e–)(2.00 V)
AS ΔGo=−-1586Kj negative ——————-reaction is sponatensous