A. use the following steps to balance the redox reaction below. al(s) ni2 (aq) ni(s) al3 (aq)
i. write the oxidation and reduction half-reactions. make sure each half-reaction is balanced for number of atoms and charge.
ii. multiply each half-reaction by the correct number in order to balance charges for the two half-reactions.
iii. add the equations and simplify to get a balanced equation.

2Al(s) +3Ni²⁺(aq) ⟶ 2Al³⁺(aq) + 3Ni(s)  

Explanation:

The unbalanced equation is

Al(s) + Ni²⁺(aq) ⟶ Ni(s) + Al³⁺(aq)

(i) Half-reactions

Al(s) ⟶ Al³⁺(aq) + 3e⁻

Ni²⁺(aq) + 2e⁻ ⟶ Ni(s)

(ii) Balance charges

2 × [Al(s) ⟶ Al³⁺(aq) + 3e⁻]

3 × [Ni²⁺(aq) + 2e⁻ ⟶ Ni(s)]

gives

2Al(s) ⟶ 2Al³⁺(aq) + 6e⁻

3Ni²⁺(aq) + 6e⁻ ⟶ 3Ni(s)

(iii) Add equations

2Al(s) ⟶ 2Al³⁺(aq) + 6e⁻

3Ni²⁺(aq) + 6e⁻ ⟶ 3Ni(s)                                        

2Al(s) +3Ni²⁺(aq) + 6e⁻ ⟶ 2Al³⁺(aq) + 3Ni(s) + 6e⁻

Simplify (cancel electrons)

2Al(s) +3Ni²⁺(aq) ⟶ 2Al³⁺(aq) + 3Ni(s)

false

because it does not have the potential to be entirely used up

because of all the things that happen around the us, many people get into arguments which sadly could get physical, but we should actually make a change for that.