Question

And electro chemical cell has the following standard cell notation:
Mg(s) | Mg2+ (aq) || Ag+(aq)| Ag(s)

Write a balanced redox reaction for the cells using the oxidation and reduction half reactions. (be sure to equalize charge by multiplying the correct number before adding and simplifying)

Answer 1

2Ag⁺(aq) + Mg(s)→ 2Ag(s) + Mg²⁺ (aq)

Further explanation

Given

Standard cell notation:

Mg(s) | Mg2+ (aq) || Ag+(aq)| Ag(s)

Required

a balanced redox reaction

Solution

At the cathode the reduction reaction occurs, the anode oxidation reaction occurs

In reaction:  

Ag⁺ + Mg → Ag + Mg²⁺  

half-reactions

• at the cathode (reduction reaction)

Ag⁺ (aq) + e⁻ ---> Ag (s)  x2

2Ag⁺ (aq) + 2e⁻ ---> 2Ag (s)

• at the anode (oxidation reaction)

Mg (s) → Mg²⁺ (aq) + 2e−

a balanced cell reaction

2Ag⁺(aq) + Mg(s)→ 2Ag(s) + Mg²⁺ (aq)

Answer 2

Answer:

2Ag⁺(aq) + Mg(s)→ 2Ag(s) + Mg²⁺ (aq)

Explanation:

a p e x :)