pure zinc metal into a solution of copper(II) sulfate, the zinc will slowly dissolve to produce zinc sulfate solution, and the copper(II) ion of the copper(II) sulfate will be converted to metallic copper. Write the unbalanced equation for this process. (Include states-of-matter under the given conditions in your answer.)

Zn(s) + CuSO4(aq) ==>ZnSO4(aq) + Cu(s)

This equation is balanced as is; therefore, I can't write an unbalanced equation and I don't think the person who made up this question can either.

Sure, here's the unbalanced equation for this process:

Zinc (s) + Copper(II) sulfate (aq) → Zinc sulfate (aq) + Copper (s)

Just remember, in this reaction, the zinc gets all mushy, dissolves into zinc sulfate solution, while the copper(II) ion, feeling a little under the weather, decides to transform into metallic copper.

The unbalanced equation for the process described can be written as:

Zinc (s) + Copper(II) sulfate (aq) → Zinc sulfate (aq) + Copper (s)

To write the unbalanced equation for this process, we need to determine the chemical formulas and states of matter of the reactants and products involved.

The reactants are pure zinc metal (Zn) and a solution of copper(II) sulfate (CuSO4). The state of matter for zinc is solid (s), while the copper(II) sulfate is in solution form (aq).

The products are zinc sulfate (ZnSO4), which is in solution form (aq), and metallic copper (Cu), which is a solid (s).

Based on this information, the unbalanced equation can be written as follows:

Zn (s) + CuSO4 (aq) → ZnSO4 (aq) + Cu (s)