Question 4: Balancing Redox Equations (5 points)
Use the following steps to balance the redox reaction below:
Mg + Au* → Mg²+ + Au
a. Write the oxidation and reduction half-reactions. Make sure each half-reaction
is balanced for number of atoms and charge. (3 points)
b. Multiply each half-reaction by the correct number, in order to balance charges
for the two half-reactions. (1 point)
c. Add the equations and simplify to get a balanced equation. (1 point)

Question

14-06-2022
Chemistry

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Question 4: Balancing Redox Equations (5 points)
Use the following steps to balance the redox reaction below:
Mg + Au* → Mg²+ + Au
a. Write the oxidation and reduction half-reactions. Make sure each half-reaction
is balanced for number of atoms and charge. (3 points)
b. Multiply each half-reaction by the correct number, in order to balance charges
for the two half-reactions. (1 point)
c. Add the equations and simplify to get a balanced equation. (1 point)

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aliasger2709 aliasger2709 · Answer 1 · 2022-06-23T16:06:32+02:00

Reactions are balanced by equating the right and the left side by stoichiometry coefficients. The redox reactions are balanced and corrected by simplifying the numbers.

What is a redox reaction?

A redox reaction is a depiction of the oxidation and the reduction of the reaction that shows the loss and the gain of the electrons by the chemical species.

The oxidation half-reaction:

Mg → Mg²⁺ + 2e⁻

The reduction half-reaction:

2Au + 2 e⁻ → 2 Au

The overall balanced reaction is:

Mg(s) + 2Au⁺ (aq) → Mg²⁺ (aq) + 2Au(s)

Therefore, the reaction is balanced by the oxidation and the reduction halves.

Learn more about redox equations here:

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