Write the total ionic and the net ionic equations for the following:

Show what you can do on your own and explain what you don't understand (in detail).

To write the total ionic and net ionic equations, you need to break down the reactants and products into their respective ions.

The given balanced equation is:
3 H2 (g) + 2 AuCl3 (aq) → 6 HCl (aq) + 2 Au (s)

To write the total ionic equation:
- Write all the compounds that are soluble (aqueous) as their individual ions.
- Write any insoluble compounds as their molecular formula.

Breaking down the reactants and products:
3 H2 (g) → 6 H+ (aq) + 6 e- (oxidation half-reaction)
2 AuCl3 (aq) → 6 Cl- (aq) + 2 Au3+ (aq) (disproportionation of Au atoms)

Note: The Au atoms in AuCl3 undergo a redox reaction, where some atoms are oxidized from a 0 oxidation state to +3 (Au3+), and the rest are reduced to elemental gold (Au).

6 HCl (aq) (already in ionic form)
2 Au (s) (solid elemental gold)

Writing the total ionic equation:
3 H2 (g) + 2 AuCl3 (aq) → 6 H+ (aq) + 6 Cl- (aq) + 2 Au (s)

To write the net ionic equation:
- Remove the spectator ions (the ions that appear on both sides of the equation and do not participate in the reaction).
- Keep only the ions and molecules that are directly involved in the reaction.

For the net ionic equation:
The spectator ions in this reaction are H+ and Cl- since they are both present on both sides of the equation.
Removing the spectator ions, we get:

Net ionic equation:
2 AuCl3 (aq) → 2 Au (s) + 6 Cl- (aq)

Therefore, the total ionic equation is: 3 H2 (g) + 2 AuCl3 (aq) → 6 H+ (aq) + 6 Cl- (aq) + 2 Au (s)
And the net ionic equation is: 2 AuCl3 (aq) → 2 Au (s) + 6 Cl- (aq)