What is the balanced chemical equation for the galvanic cell reaction expressed using shorthand notation below?

Al(s)|Al3+(aq)||Ni2+(aq)|Ni(s)

2 Al(s) + 3 Ni2+(aq)-->2 Al3+(aq) +3 Ni(s)

is this correct?

Al(s) + Ni^+2 ==>Al^+3 + Ni(s)

I will let you balance it. Remember that the electron exchange must balance as well as the ions themselves.
It may be easier for you to look at the two half cells.
Al(s) ==> Al^+3 + 3e
Ni^+2 + 2e ==> Ni(s)

yes

To write the balanced chemical equation for the galvanic cell reaction, we need to identify the half-reactions occurring at each electrode.

In shorthand notation:
- The left side of the vertical line represents the anode, where oxidation occurs.
- The right side of the vertical line represents the cathode, where reduction occurs.

Given:
Anode: Al(s) | Al3+(aq)
Cathode: Ni2+(aq) | Ni(s)

Step-by-step explanation:

1. Identify the half-reactions at each electrode:
Anode: Al(s) ⟶ Al3+(aq) + 3e-
Cathode: Ni2+(aq) + 2e- ⟶ Ni(s)

2. Balance the number of atoms in each half-reaction:
Anode: 2Al(s) ⟶ 2Al3+(aq) + 6e-
Cathode: 3Ni2+(aq) + 6e- ⟶ 3Ni(s)

3. Multiply the half-reactions by appropriate coefficients to make the number of electrons equal on both sides:
Anode: 2Al(s) ⟶ 2Al3+(aq) + 6e-
Cathode: 3Ni2+(aq) + 6e- ⟶ 3Ni(s)

4. Combine the half-reactions and cancel out the electrons to obtain the balanced overall cell reaction:
2Al(s) + 3Ni2+(aq) ⟶ 2Al3+(aq) + 3Ni(s)

Thus, the balanced chemical equation for the galvanic cell reaction, expressed using shorthand notation, is:
2Al(s) + 3Ni2+(aq) ⟶ 2Al3+(aq) + 3Ni(s)