What are the equations for these two equations? Not net ionic equations.

a) Nickel (II) chloride and iron
b) Sodium and water

Fe(s) + NiCl2(aq) ==> FeCl2(aq) + Ni(s)

2Na(s) + 2H2O(l) ==> 2NaOH(aq) + H2(g)

You need the activity series to do these. Here is a site that I like.
http://www.files.chem.vt.edu/RVGS/ACT/notes/activity_series.html

This site tells you that any metal will displace the ion of a metal BELOW it in the series. Fe is above Ni; therefore, Fe displaces Ni^2+ in NiCl2. Na is above H; therefore, Na displaces H^+ in H2O.
If you had Ni + FeCl2 ==> you would write No reaction BECAUSE Ni is BELOW Fe so Ni will not displace Fe^2+

To determine the equations for these two reactions, we need to identify the chemical formulas and the products formed when nickel (II) chloride reacts with iron and when sodium reacts with water.

a) Nickel (II) chloride and iron:
Start by writing the chemical formula for each reactant:
- Nickel (II) chloride: NiCl2
- Iron: Fe

Next, we need to determine the products formed when these two substances react. In this case, nickel is a cation with a charge of +2 (Ni2+), and chloride is an anion with a charge of -1 (Cl-). Iron is a metal and can lose two electrons to achieve a stability of Fe2+.

The balanced equation for this reaction is:
2NiCl2 + Fe → 2Ni + FeCl2

b) Sodium and water:
Again, begin by writing the chemical formula for each reactant:
- Sodium: Na
- Water: H2O

Sodium is a metal and can lose one electron to achieve a stability of Na+, while water is a compound consisting of hydrogen (H) and oxygen (O).

The balanced equation for this reaction is:
2Na + 2H2O → 2NaOH + H2

In both equations, the coefficients have been adjusted to ensure that the number of atoms of each element is balanced on both sides of the equation. The resulting equations represent the chemical reactions that occur between the given reactants.