Lab Report Comparative Reactivity of Metals PDF

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Comparative Reactivity of Metals By: Jonathan Pilafas (performed on 10/1/2018)

Purpose: The objective of the “Comparative Reactivity of Metals” portion of this lab is to record the reactivity of three different metals in aqueous solutions.

References: 1. “Laboratory Experiments for Chemistry 121” - Harper College 2. http://dept.harpercollege.edu/chemistry/msds1/msds.html

Reagents:

Name

Formula

Magnesium Sulfide

MgSO₄

Copper Sulfate

CuSO₄

Zinc Sulfate

ZnSO₄

Procedure: To begin the experiment, collect a reasonable amount of M  gSO₄, CuSO₄, and

ZnSO₄, as well as three pieces of solid Magnesium, Copper, and Zinc. Pour 1 mL of MgSO₄, CuSO₄, and ZnSO₄ into three test tubes each. Place a different metal in each test tube for each reactant. Observe the initial reactions of these reactants, and observe

them again after 10 minutes passes by. Using the observations that have been recorded from the previous prompt, determine the order of reactivity of these reactants.

Data:

Metal

MgSO

ZnSO

CuSO

Mg

Slightly cloudy

N/A

N/A

Zn

N/A

Cloudy, powdery, white

Cloudy, powdery, white

Cu

Light brown

Black

N/A

Molecular Equations: Magnesium: Mg (s) + MgSO₄ (aq) → Mg (aq) + MgSO₄ (aq) Mg (s) + CuSO₄ (aq) → Mg (s) + CuSO₄ (aq) (no reaction) Mg (s) + ZnSO₄ (aq) → Mg (s) + ZnSO₄ (aq) (no reaction)

Copper: Cu (s) + MgSO₄ (aq) → Mg (aq) + CuSO₄ (aq) Cu (s) + CuSO₄ (aq) → Cu (s) + CuSO₄ (aq) (no reaction) Cu (s) + ZnSO₄ (aq) → Cu (s) + ZnSO₄ (aq) (no reaction)

Zinc: Zn (s) + MgSO₄ (aq) → Zn (s) + MgSO₄ (aq) (no reaction) Zn (s) + CuSO₄ (aq) → Cu + ZnSO₄ Zn (s) + ZnSO₄ (aq) → Zn + ZnSO₄

Ionic Equations: Magnesium: Mg2+ (s) + M  g2+ (aq) + SO₄2- (aq) → Mg2+ (aq) + Mg2+ (aq) + SO₄2- (aq) Mg2+ (s) + C  u2+ (aq) + SO₄2- (aq) → Mg2+ (s) + Cu2+ (aq) SO₄2- (aq) (no reaction) Mg2+ (s) + Z  n2+ (aq) + SO₄2- (aq) → Mg2+ (s) + Zn2+ (aq) + SO₄2- (aq) (no reaction)

Copper: Cu2+ (s) + Mg2+ (aq) + SO₄2- (aq) → Mg2+ (aq) + Cu2+ (aq) SO₄2- (aq) Cu2+ (s) + Cu2+ (aq) + SO₄2- (aq) → Cu2+ (s) + Cu2+ (aq) SO₄2- (aq) (no reaction) Cu2+ (s) + Zn2+ (aq) + SO₄2- (aq) → Cu2+ (s) + Zn2+ (aq) + SO₄2- (aq) (no reaction)

Zinc: Zn2+ (s) + Mg2+ (aq) + SO₄2- (aq) → Zn2+ (s) + Mg2+ (aq) + SO₄2- (aq) (no reaction) Zn2+ (s) + Cu2+ (aq) + SO₄2- (aq) → Cu2+ (aq) + Zn2+ (aq) + SO₄2- (aq) Zn2+ (s) + Zn2+ (aq) SO₄2- (aq) → Zn2+ (aq) + Zn2+ (aq) + SO₄2- (aq)

Net Ionic Equations: Magnesium: Mg2+ (s) → Mg2+ (aq) No reaction No reaction

Copper: Cu2+ (s) + → Cu2+ (aq)

No reaction No reaction

Zinc: No reaction Zn2+ (s) + → Zn2+ (aq) Zn2+ (s) →  Zn2+ (aq)

Discussion:

As I tested the reactivity of three different metals in three different aqueous solutions, I determined an activity series of the metals I tested. While testing magnesium, I concluded that magnesium was only reactive with the reactant MgS  O₄. While testing copper, I concluded that copper was only reactive with the reactant MgS  O₄. Lastly, while testing zinc, I concluded that zinc was reactive with the reactants ZnSO₄ and C  uSO₄. I came to these conclusions for all

three of these metals by making observations when combining them with reactants MgSO₄, CuSO₄, and ZnSO₄.

Conclusion: As a result of this lab, I have concluded that metals magnesium and copper are reactive with the reactant MgSO₄. I have also concluded that zinc is reactive with the reactants ZnSO₄ and CuSO₄. By creating organized and thorough directions, following them extensively, and observing them numerous times throughout the experiment, I have determined solid evidence that these metals are indeed reactive with the reactants that have been previously listed....