Current is applied to a molten mixture of AgF, ZnCl2, and AlBr3. What is produce

Question

Current is applied to a molten mixture of AgF, ZnCl2, and AlBr3.

What is produced at the cathode?

F2

Ag

Br2

Cl2 <<<< I think this is the answer

Al

Zn

What is produced at the anode?

Al <<< I think this is the answer

Zn

Br2

F2

Ag

Cl2

HINT:

Standard potentials may be found here. Although these potentials are given for aqueous half-reactions, we can infer the relative reduction and oxidation potentials of molten ions from their aqueous counterparts. https://sites.google.com/site/chempendix/oxidation-potentials

This is my last sapling problem today!

Explanation / Answer

Reduction takes place at cathode.

We know that reduction potential for

Ag+ + e- ---> Ag ..... E = 0.8 V

Zn2+ + 2e- ----> Zn ... E = - 0.76 V

Al3+ + 3e- -----> Al ..... E = -1.66 V

We see that reduction potential for Ag is highest. Hence Ag will deposit at the cathode.

Oxidation takes place at anode

Oxidation potentials are:

2F- -----> F2 + 2e- ..... E = - 2.87 V

2Cl- -----> Cl2 + 2e- .... E = - 1.36 V

2Br- -----> Br2 + 2e- ..... E = -1.07 V

Oxidation potential for Br- is the highest. Hence Br2 will be produced at the anode.

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