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Lab Report Electrochemical Cell Experiment

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Lab report - Electrochemical Cells
Name: Assiya Meirmanova
Group: 13
Lab partner: Kamilya Nurlanova
Aim
The main purpose of the practical is to find the emf of the cell and discover how emf changes within a different concentration which also helps to acquire a knowledge about Galvanic cell and it`s setup.
Introduction
This experiment is designed to discover the potential of electrochemical cells. It requires a little understanding about electrochemical cells since experiment is concentrated on practice rather than on theoretical aspects. An electrochemical cell is based on an oxidation-reduction reaction (redox). Oxidation and reduction are the most wide spread examples of chemical reactions that occurs in nature, it involves the transfer …show more content…

Two pieces of zinc and copper were attached to the voltmeter. 40mL of solution was gently dispensed into two beakers. Salt bridge, made of piece of paper soaked in saturated potassium nitrate, was placed between the solutions. Voltage potential indicated on the voltmeter was recorded. Finally, emery paper was used to clean the consistent foils to make them convenient for the further practical.
Experiment 3: Constructing a zinc/iron cell
The same approach was applied to those half-cells. Two pieces of Zn and Fe were attached to the voltmeter. Then a contaminated salt bridge was replaced by cleaner one. 40 ml of iron solution was dispensed into empty beaker and potential voltage was recorded.
Experiment 4: Constructing an iron/copper cell
The piece of the metal and the solution of the zinc were replaced with copper`s. Clean salt bridge was soaked in saturated potassium nitrate and placed between two half-cells. Then potential voltage was recorded.
Experiment 5: Effect of concentration on
Zn and Cu metals were cleaned with emery paper, the solution of the 1M CuSO4 was changed with 0.001M CuSO4, 0.01M CuSO4 and 0.1M CuSO4 respectively, piece of metals were attached to the wire and observed data was recorded.
Results
Observed records from Cu2+ and Zn reactions
Solution Color turned from blue to brown
Tube The temperature changed from cold to warm
Solid Solid precipitation is …show more content…

Based on the recorded data, it can be concluded that, zinc metal is much oxidized to zinc ion, so zinc plays an anode role and it loses electron, while two cupper ions are reduced through the addition of two electrons to form solid copper. 3) Fe2+ (1.00M) + 2e → Fe(s) E= -044 cathode Zn(s) → Zn2+ (aq) + 2ē) E = −0.76 V anode 4) Cu2+ (aq), 1.00M + 2e → Cu(s) E = +0.34 V cathode Fe2+ (aq), 1.00M + 2e → Fe(s) E= -044 anode
In third experiment, Fe2+ had a greater tendency to be reduced than Zn2+, iron electrode was defined as cathode and zinc electrode was defined as anode, and zinc metal was oxidized to form an zinc ion with a +2 charge; whereas in fourth experiment Cu(s) was the reducing agent, as it caused Fe+ to gain electrons.
5) The effect of Cu

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