What type of reactions are these?

Acid-base? Oxidation/Reduction? Precipitation?

1) Zn (s) + 2 HCl (aq) -> ZnCl2 (aq) + H2 (g)

2) Fe (s) + CuSO4 (aq) -> FeSO4 (aq) + Cu (s)

3) Fe (s) + Cu(NO)2 (aq) -> Fe(NO3)2 (aq) + Cu(s)

To determine the type of reactions in the given equations, we need to examine the reactants and products involved. Here's how you can identify each type:

1) Zn (s) + 2 HCl (aq) -> ZnCl2 (aq) + H2 (g)

In this equation, zinc (Zn) reacts with hydrochloric acid (HCl) to produce zinc chloride (ZnCl2) and hydrogen gas (H2). This is an example of an acid-base reaction as the acid (HCl) donates protons (H+) to the zinc, forming an ionic compound (ZnCl2) and releasing hydrogen gas.

2) Fe (s) + CuSO4 (aq) -> FeSO4 (aq) + Cu (s)

This equation represents the reaction between iron (Fe) and copper(II) sulfate (CuSO4). Iron displaces copper from copper(II) sulfate, resulting in the formation of iron(II) sulfate (FeSO4) and elemental copper (Cu). This is an example of a single displacement reaction, specifically an oxidation/reduction (redox) reaction. Iron loses electrons and is oxidized (it goes from 0 to +2 oxidation state), while copper gains electrons and is reduced (it goes from +2 to 0 oxidation state).

3) Fe (s) + Cu(NO)2 (aq) -> Fe(NO3)2 (aq) + Cu(s)

In this equation, iron (Fe) reacts with copper(II) nitrate (Cu(NO3)2) to produce iron(II) nitrate (Fe(NO3)2) and elemental copper (Cu). Similar to the previous equation, this is also a single displacement reaction and a redox reaction. Iron is oxidized (loses electrons) while copper is reduced (gains electrons).

So, to summarize, the reactions in these equations are as follows:
1) Acid-base reaction
2) Oxidation/reduction (redox) reaction
3) Oxidation/reduction (redox) reaction