Question
Mg(s)/Mg^2+(aq)//Al^3+(aq)/Al(s)
1. Give the overall balanced cell reaction
2. Provide the half reaction for the galvanic cell line notation
3. Calculate the E°cell for the galvanic cell and comment on its value
1. Give the overall balanced cell reaction
2. Provide the half reaction for the galvanic cell line notation
3. Calculate the E°cell for the galvanic cell and comment on its value
Answers
GPT 3.5
1. Overall balanced cell reaction: Mg(s) + 2Al^3+(aq) -> Mg^2+(aq) + 2Al(s)
2. Half reactions:
Anode: Mg(s) -> Mg^2+(aq) + 2e-
Cathode: 2Al^3+(aq) + 6e- -> 2Al(s)
Galvanic cell line notation: Mg(s)|Mg^2+(aq) || Al^3+(aq)|Al(s)
3. E°cell = E°cathode - E°anode
E°cell = -1.67 V - (-2.37 V) = 0.70 V
The positive E°cell value indicates that the cell reaction is spontaneous and has a driving force to proceed in the forward direction. This means that the reduction of Al^3+ to Al at the cathode is favored over the oxidation of Mg to Mg^2+ at the anode.
2. Half reactions:
Anode: Mg(s) -> Mg^2+(aq) + 2e-
Cathode: 2Al^3+(aq) + 6e- -> 2Al(s)
Galvanic cell line notation: Mg(s)|Mg^2+(aq) || Al^3+(aq)|Al(s)
3. E°cell = E°cathode - E°anode
E°cell = -1.67 V - (-2.37 V) = 0.70 V
The positive E°cell value indicates that the cell reaction is spontaneous and has a driving force to proceed in the forward direction. This means that the reduction of Al^3+ to Al at the cathode is favored over the oxidation of Mg to Mg^2+ at the anode.
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