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

b. Multiply each half-reaction by the correct number, in order to balance charges for the two half-reactions.

c. Add the equations and simplify to get a balanced equation.

To balance the redox reaction, follow these steps:

a. Write the oxidation and reduction half-reactions:

First, identify the species that are being oxidized and reduced. In this case, magnesium (Mg) is being oxidized from a neutral state (0 charge) to a +2 charge, and gold (Au+) is being reduced from a +1 charge to a neutral state (0 charge).

Oxidation half-reaction:
Mg -> Mg2+ (balanced for atoms)

Reduction half-reaction:
Au+ -> Au (balanced for atoms)

Now, balance the charges in each half-reaction:

Oxidation half-reaction:
Mg -> Mg2+ + 2e- (balanced for charge)

Reduction half-reaction:
Au+ + e- -> Au (balanced for charge)

b. Multiply each half-reaction by the correct number to balance charges for the two half-reactions:

Multiply the oxidation half-reaction by 2 to balance the number of electrons:

2Mg -> 2Mg2+ + 4e-

Now, the number of electrons in the oxidation and reduction half-reactions is balanced.

c. Add the equations and simplify to get a balanced equation:

Add the oxidation and reduction half-reactions:

2Mg + Au+ -> 2Mg2+ + Au

Simplify the equation, if needed. In this case, the equation is already balanced, so no further simplification is required.

The balanced equation for the redox reaction is:

2Mg + Au+ -> 2Mg2+ + Au

Mg to Mg2+ loses 2 electrons

Au+ to Au gains one electron. So 2Au for each Mg

Mg yields Mg+ +2e
Au+ + e yields Au

so multiply the second equation by 2

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