Chemistry Practicals Class 12
Determination of the EMF of a Daniell Cell
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About Simulation
- You will understand the terms electrochemical cell, electrolytic cell, Daniell cell, salt bridge, standard electrode potential, and EMF.
- In this electrochemistry experiment, you will acquire the skills required to construct a Daniell cell.
- You will understand the significance of the salt bridge.
- You will be able to calculate the electrode potential of a half-cell and full-cell using the Nernst equation in the competitive exams.
- You will acquire the skills to measure the EMF of a cell by viewing animations in the Chemistry virtual lab.
- Using our e-learning product, you will understand how the electrode potential of a given cell varies with the concentration of electrolytes in the anodic and cathodic half-cell.
Simulation Details
Description
Electrochemistry is the study of the interchange of chemical energy and electrical energy. The process of conversion of chemical energy into electrical energy is called an electrochemical reaction. Hence, the cells which convert chemical energy into electrical energy are known as electrochemical cells. Whereas the reverse process is called electrolytic reaction or electrolysis, and devices that undergo a chemical reaction with the aid of electricity are called electrolytic cells.
The best example of an electrochemical cell is the Daniell cell, in which copper and zinc electrodes are immersed in a solution of copper sulphate and zinc sulphate, respectively. Zinc metal acts as an anode, and copper acts as a cathode. Oxidation occurs at the anode with the loss of electrons and reduction at the cathode with the gain of electrons. The transfer of electrons occurs from the anode to cathode and the circuit completes. The potential difference between the two electrodes is called emf or cell potential. It is measured in Volts. The spontaneity of the reaction depends on the reactivity of metals. The cell reaction for the Daniell cell is $$\mathrm{Zn}{(\mathrm{s})}+\mathrm{Cu}{(\mathrm{aq})}^{2+} \rightarrow \mathrm{Zn}{(\mathrm{aq})}^{2+}+ \mathrm{Cu}\mathrm{(s)}$$
Nernst’s equation to calculate the emf of Daniell cell is
$$\mathrm{E_{cell}=E_{cell}^0-\frac{RT}{nF}ln\frac{[Zn^{2+}]}{[Cu^{2+}]}}$$
Watch this video to learn more about chemistry.
Requirements for this Science Experiment
⦁ Voltmeter ⦁ Salt Bridge ⦁ Zinc and copper Electrodes ⦁ Connecting Wires ⦁ Sand Paper ⦁ Beakers ⦁ Graduated Cylinder ⦁ Weighing Balance ⦁ Weighing Bottle ⦁ Spatula ⦁ Glass Rod
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