Question

write a balanced net ionic equation for the redox reaction of ag2s and al metal that produces ag metal and al(oh)3.

Answer 1

The balanced net ionic equation for the redox reaction between Ag2S and aluminum metal involves the reduction of Ag+ ions and the oxidation of Al metal, resulting in the formation of Ag metal and Al(OH)3.

Step-by-step explanation:

To write a balanced net ionic equation for the redox reaction between Ag2S and aluminum metal, we split the reaction into two half-reactions: the oxidation of Al and the reduction of Ag+. The Ag2S reactant will dissociate into two Ag+ ions and one S2- ion.

The half-reactions are as follows:

• Ag+ + e- → Ag (Reduction half-reaction)
• Al → Al3+ + 3e- (Oxidation half-reaction)

To balance the electrons, we multiply the reduction half-reaction by 3:

• 3Ag+ + 3e- → 3Ag

Combining the balanced half-reactions, we have:

3Ag+ + Al → 3Ag + Al3+ + 3OH-

Since there was an S2- ion from Ag2S, we need to balance that with hydroxide ions to form aluminum hydroxide:

Al3+ + 3OH- → Al(OH)3

Combining all parts, the net ionic equation is:

3Ag+ + Al + 3S2- + 9OH- → 3Ag + 3Al(OH)3

This equation shows the conversion of silver sulfide (Ag2S) and aluminum metal to silver metal (Ag) and aluminum hydroxide (Al(OH)3) in a redox reaction.