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Introduction –
According to http://www.shodor.org/unchem/advanced/redox/index.html, “fundamentally, redox reactions are a family of reactions that are concerned with the transfer of electrons between species.” These reactions occur when one reactant has excess electrons to offer and another reactant is in need of gaining electrons, such as to neutralize. Within these reactions, oxidation occurs when a substance loses electrons, and thus, reduction occurs when a substance gains electrons. Oxidation cannot occur without reduction and vice versa. The substance being oxidized is labeled as the reducing agent, because its oxidation is what allows the other substance to be reduced. With this being said, the substance that is reduced is labeled as the oxidizing agent, because its oxidation is what allows for reduction to occur.

Purpose –
The object of this experiment is to carry out a number of redox reactions involving common oxidants and reductants. Changes that occur will be observed and interpreted in terms of the reactants occurring, and balanced equations will be written, using the half equations method.

Materials –
A 2 cm depth of aqueous copper sulfate, a small piece of granulated zinc, A 2 cm depth of aqueous potassium dichromate (VI), aqueous sulfur dioxide, a small piece of magnesium ribbon, and a 3 cm depth of dilute sulfuric acid, a 2 cm depth of aqueous ethanedioic acid, Bunsen burner, a 1 cm depth of limewater, a 2 cm depth of potassium permanganate(VII) solution, a 2 cm depth of hydrogen peroxide, a glowing splint, a 2 cm depth of water, a spatula full of calcium, a lighted splint, 6 test tubes.

Procedure to keep it controlled –
• The entire experiment will be performed in the same room and under the same conditions such as temperature and light intensity.

Procedure –
A 2 cm depth of aqueous copper sulfate was put in a test tube and a small piece of...