Consider the following galvanic cell: Mg(s)|Mg^2+ (aq)| |Al^3+ (aq)|Al(s) Standa

Question

Consider the following galvanic cell: Mg(s)|Mg^2+ (aq)| |Al^3+ (aq)|Al(s) Standard Reduction Potentials: Mg^2+ +2e^1- rightarrow Mg(s) E^o -2.37V Al^3+3e^1- rightarrow Al(s) E^o-1.66V Give the equation for the spontaneous cell reaction that produces charge flow. Indicate which substance is oxidized and which is reduced in this reaction. Identify the anode and the cathode electrodes for this cell. Calculate the E_cell^o. How will the potential difference (voltage) of the galvanic cell Cu(s) + 2Ag^1+ (aq) rightarrow Cu^2+ (aq) + 2Ag(s) be affected by the addition of Nacl(aq)? Explain. How does increasing the mass of the anode affect the voltage? Justify your response. Consider the reduction potentials: Na^1+ e^1+ rightarrow Na(s) E^o -2.71 V 2H_2O + 2e^1- rightarrow H_2 + 2OH^1- E^o -2.37 V The electrolysis of aqueous NaCl does not produce metallic sodium. Explain

Explanation / Answer

(a) Spantaneous redox reaction:

3 Mg(s) + 2 Al3+ (aq.) -------------> 3 Mg2+ (aq.) + 2 Al (s)

* The ion with smaller electrode potential undergoes oxidation and the other undergoes reduction.

(b)

The species that undergo oxidation is Mg(s)

The species that undergoes reduction is Al3+

(c) E0cell = E0cathode - E0anode

E0cell = - 1.66 - ( - 2.37) = 0.71 V

(d)

Addition NaCl cuase the folloing reaction to occur,

NaCl (aq.) + Ag+ (aq.) -----------> AgCl (s) + Cl- (aq.)

SO, it decreases the concentration of Ag+ ions which cause to decrease the cell potential.

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