Given the galvanic cell: (Anode) Mg / Mg 2+(aq) // Zn2+(aq) / Zn (Cathode) with E˚ = +1.61 V Know that 0 (Zn2+/Zn) = – 0.76 V, calculate the 0 (Mg2+/Mg)
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Given : At cathode - E°(Zn2+/Zn ) = -0.76 V ,
E°cell = +1.61 V .
Find : E° (Mg2+/Mg) .
Solution :
- A galvanic cell is given which is a electrochemical cell that converts chemical energy of spontaneous redox reactions into the electrical energy.
- In this question we have given the value of E° (Zn2+/Zn ) , it is a anode terminal means where the oxidation takes place .
- While we have to find out the E° (Mg2+/Mg) , it is a cathode terminal means where the reduction takes place .
- As we know the formula of E°cell from where we can find out the value of E° (Mg2+/Mg).
- So, E°cell = E°cathode - E° anode
= E°(Zn2+/Zn ) - E° (Mg2+/Mg)
=> 1.61 = -0.76 -E° (Mg2+/Mg)
=> E° (Mg2+/Mg) = -0.76-1.61 = -2.37 V
- So, the value of E° (Mg2+/Mg) is -2.37 V.
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