Write the balanced molecular and net ionic equation for the reaction that occurs when the contents of the two beakers are added together. (use the lowest possible coefficients. include states-of-matter under satp conditions in your answer.)

1) hydrochloric acid with nickel:

Balanced molecular equation: Ni (s) + 2HCl (aq) → NiCl₂ (aq) + H₂ (g).

Ionic equation: Ni (s) + 2H⁺ (aq) + 2Cl⁻ (aq) → Ni²⁺ (aq) + 2Cl⁻ (aq) + H₂ (g).

Net ionic equation: Ni (s) + 2H⁺ (aq) → Ni²⁺ (aq) + H₂ (g).

Nickel is oxidized from oxidation number 0 (Ni) to oxidation number + 2, hydrogen is reduced from oxidation number + 1 to oxidation number 0 (H₂).

2) sulfuric acid with iron:

Balanced molecular equation: Fe (s) + H₂SO₄ (aq) → FeSO₄ (aq) + H₂ (g).

Ionic equation: Fe (s) + 2H⁺ (aq) + SO₄²⁻ (aq) → Fe²⁺ (aq) + SO₄²⁻ (aq) + H₂ (g).

Net ionic equation: Fe (s) + 2H⁺ (aq) → Fe²⁺ (aq) + H₂.

Iron is oxidized from oxidation number 0 (Fe) to oxidation number + 2, hydrogen is reduced from oxidation number + 1 to oxidation number 0 (H₂).

3) hydrobromic acid with magnesium:

Balanced molecular equation: Mg (s) + 2HBr (aq) → MgBr₂ (aq) + H₂ (g).

Ionic equation: Mg (s) + 2H⁺ (aq) + 2Br⁻ (aq) → Mg²⁺ (aq) + 2Br⁻ (aq) + H₂ (g).

Net ionic equation: Mg (s) + 2H⁺ (aq) → Mg²⁺ (aq) + H₂ (g).

Magnesium is oxidized from oxidation number 0 (Mg) to oxidation number + 2, hydrogen is reduced from oxidation number + 1 to oxidation number 0 (H₂).

4) acetic acid with zinc:

Balanced molecular equation: Zn (s) + 2CH₃COOH (aq) → (CH₃COO) ₂Zn (aq) + H₂ (g).

Ionic equation: Zn (s) + 2H⁺ (aq) + 2CH₃COO⁻ (aq) → Zn²⁺ (aq) + 2CH₃COO⁻ (aq) + H₂ (g).

Net ionic equation: Zn (s) + 2H⁺ (aq) → Zn²⁺ (aq) + H₂ (g).

Zinc is oxidized from oxidation number 0 (Zn) to oxidation number + 2 (Zn²⁺), hydrogen is reduced from oxidation number + 1 to oxidation number 0 (H₂).