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kolezko [41]
3 years ago
7

A chemist designs a galvanic cell that uses these two half-reactions:

Chemistry
1 answer:
Nonamiya [84]3 years ago
4 0

Answer :

(a) Reaction at anode (oxidation) : 4Fe^{2+}\rightarrow 4Fe^{3+}+4e^-  

(b) Reaction at cathode (reduction) : O_2+4H^++4e^-\rightarrow 2H_2O  

(c) O_2+4H^++4Fe^{2+}\rightarrow 2H_2O+4Fe^{3+}

(d) Yes, we have have enough information to calculate the cell voltage under standard conditions.

Explanation :

The half reaction will be:

Reaction at anode (oxidation) : Fe^{2+}\rightarrow Fe^{3+}+e^-     E^0_{anode}=+0.771V

Reaction at cathode (reduction) : O_2+4H^++4e^-\rightarrow 2H_2O     E^0_{cathode}=+1.23V

To balance the electrons we are multiplying oxidation reaction by 4 and then adding both the reaction, we get:

Part (a):

Reaction at anode (oxidation) : 4Fe^{2+}\rightarrow 4Fe^{3+}+4e^-     E^0_{anode}=+0.771V

Part (b):

Reaction at cathode (reduction) : O_2+4H^++4e^-\rightarrow 2H_2O     E^0_{cathode}=+1.23V

Part (c):

The balanced cell reaction will be,

O_2+4H^++4Fe^{2+}\rightarrow 2H_2O+4Fe^{3+}

Part (d):

Now we have to calculate the standard electrode potential of the cell.

E^o=E^o_{cathode}-E^o_{anode}

E^o=(1.23V)-(0.771V)=+0.459V

For a reaction to be spontaneous, the standard electrode potential must be positive.

So, we have have enough information to calculate the cell voltage under standard conditions.

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