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Ad libitum [116K]
3 years ago
5

Consider a galvanic cell in which Al 3 + Al3+ is reduced to elemental aluminum and magnesium metal is oxidized to Mg 2 + Mg2+ .

Write the balanced half-cell reactions that take place at the cathode and at the anode.

Chemistry
2 answers:
valina [46]3 years ago
8 0

Explanation:

Below is an attachment containing the solution.

olga nikolaevna [1]3 years ago
5 0

Answer:

Anode:

3Mg(s) ----------> 3Mg2+(aq) + 6e

Cathode:

2Al3+(aq) +6e ---------> 2Al(s)

Explanation:

Anode:

3Mg(s) ----------> 3Mg2+(aq) + 6e

Cathode:

2Al3+(aq) +6e ---------> 2Al(s)

Magnesium is more electro positive than aluminum hence it functions as the anode. Six electrons are lost/gained in the redox process as shown in the oxidation and reduction half reaction equations above. Magnesium is oxidized to magnesium ion while aluminum is reduced to elemental aluminum.

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Please help make sure its correct thanks
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<h3>Further explanation</h3>

13.02 g sample of Cobalt , then mol Co(MW=58.933 g/mol) :

\tt mol=\dfrac{mass}{Ar}=\\\\mol=\dfrac{13.02~g}{58.933}\\\\mol=0.221

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\tt =mass~metal~iodide-mass~Cobalt\\\\=97.12-13.02\\\\=84.1~g

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\tt \dfrac{84.1}{126.9045}=0.663

mol ratio of Cobalt and Iodine in the compound :

\tt 0.221\div 0.663=1\div 3

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