Verified answer

(a)

standard electrode potentials you need to know are:

Cl₂(g) + 2e⁻ ⇄ 2Cl⁻(aq) , E° = + 1.36V

Sn²⁺(aq) + 2e⁻ ⇄ Sn(s) , E° = - 0.14V

half reactions with potentials

reduction

Cl₂(g) + 2e⁻ ⇄ 2Cl⁻(aq) , E° = + 1.36V

oxidation

Sn(s) ⇄ Sn²⁺(aq) + 2 e⁻ , E° = + 0.14V

so overall reaction

Cl₂(g) + Sn(s) ⇄ 2 Cl⁻(aq) + Sn²⁺(aq) ,

has cell potential

E° = + 1.36V + 0.14V = + 1.50V

(b)

standard electrode potentials you need to know are:

Sn²⁺(aq) + 2e⁻ ⇄ Sn(s) , E° = - 0.14V

Zn²⁺(aq) + 2e⁻ ⇄ Zn(s) , E° = - 0.76V

half reactions with potentials

reduction

Sn²⁺(aq) + 2e⁻ ⇄ Sn(s) , E° = - 0.14V

oxidation

Zn(s) ⇄ Zn²⁺(aq) + 2e⁻ , E° = + 0.76V

so overall reaction

Sn²⁺(aq) + Zn(s) ⇄ Sn(s) + Zn²⁺(aq) ,

has cell potential

E° = - 0.14V + 0.76V = + 0.62V

(c)

standard electrode potentials you need to know are:

Cu²⁺(aq) + e⁻ ⇄ Cu⁺(aq) , E° = + 0.16V

Cu⁺(aq) + e⁻ ⇄ Cu(s) , E° = + 0.52V

half reactions with potentials

reduction

Cu⁺(aq) + e⁻ ⇄ Cu(s) , E° = + 0.52V

oxidation

Cu⁺(aq) ⇄ Cu²⁺(aq) + e⁻, E° = - 0.16V

so overall reaction

2Cu⁺(aq) ⇄ Cu(s) + Cu²⁺(aq) ,

has cell potential

E° = + 0.52V - 0.16V = + 0.36V

(d)

standard electrode potentials you need to know are:

Mg²⁺(aq) + 2e⁻ ⇄ Mg(s) , E° = - 2.36V

I₂(s) + 2e⁻ ⇄ 2I⁻(aq) , E° = + 0.54V

half reactions with potentials

reduction

I₂(s) + 2e⁻ ⇄ 2I⁻(aq) , E° = + 0.54V

oxidation

Mg(s) ⇄ Mg²⁺(aq) + 2e⁻ , E° = + 2.36V

so overall reaction

I₂(s) + Mg(s) ⇄ 2I⁻(aq) + Mg²⁺(aq)

which is the same as

I₂(s) + Mg(s) ⇄ MgI₂(aq)

has cell potential

E° = + 0.54V + 2.36V = + 2.90V

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