Electrochemistry is the study of the relationship between electricity and chemical reactions. In this blog we will find the most important questions and answers of Electrochemistry Class 12 NCERT Solutions
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What is the difference between anode and cathode?
The anode is the electrode where oxidation occurs, while the cathode is the electrode where reduction occurs. Oxidation is the process of losing electrons, while reduction is the process of gaining electrons. In an electrochemical cell, electrons flow from the anode to the cathode, and ions move through the solution or salt bridge to maintain electrical neutrality.
Define standard electrode potential.
Standard electrode potential is the potential difference between an electrode and a standard hydrogen electrode (SHE) under standard conditions. Standard conditions refer to a temperature of 25°C, a pressure of 1 atm, and a concentration of 1 M for all species in the cell. The standard electrode potential of an electrode can be used to predict the direction and magnitude of the electron transfer reaction occurring at the electrode.
What is the function of the salt bridge in an electrochemical cell?
The salt bridge in an electrochemical cell provides a pathway for the movement of ions between the two half-cells, maintaining electrical neutrality. The salt bridge contains an electrolyte solution that allows the exchange of cations and anions between the two half-cells, preventing the buildup of charge and the cessation of the redox reaction.
What is the Nernst equation?
The Nernst equation is an equation that relates the standard electrode potential of an electrode to the concentrations of the reactants and products in the cell. The equation is E = E° - (RT/nF)ln(Q), where E is the electrode potential, E° is the standard electrode potential, R is the gas constant, T is the temperature, n is the number of electrons transferred in the reaction, F is the Faraday constant, and Q is the reaction quotient.
What is Faraday's law of electrolysis?
Faraday's law of electrolysis states that the amount of a substance produced or consumed at an electrode during electrolysis is directly proportional to the amount of charge passed through the cell. The relationship can be expressed as n = Q/F, where n is the number of moles of substance produced or consumed, Q is the charge passed through the cell, and F is the Faraday constant.
What is the role of a reference electrode in electrochemistry?
A reference electrode is used as a standard for measuring the electrode potential of other electrodes. The reference electrode has a known and stable potential that is used as a reference point for measuring the potential of other electrodes. Examples of reference electrodes include the standard hydrogen electrode (SHE) and the silver/silver chloride electrode.
Can you store copper sulphate solutions in a zinc pot?
Zinc is more reactive than copper. Therefore, zinc can displace copper from its salt solution. If copper sulphate solution is stored in a zinc pot, then zinc will displace copper from the copper sulphate solution.
Hence, copper sulphate solution cannot be stored in a zinc pot.
What is meant by overpotential?
Overpotential is the extra potential required to drive a reaction at an electrode due to the resistance of the electrode surface. The resistance can be caused by factors such as the nature of the electrode material, the concentration of the reactants, and the temperature of the solution.
What is the difference between primary and secondary cells?
Primary cells are non-rechargeable cells that generate electrical energy from chemical reactions, while secondary cells are rechargeable cells that can be recharged by passing an electric current through them. Examples of primary cells include dry cells, alkaline cells, and lithium-ion cells, while examples of secondary cells include lead-acid batteries, nickel-cadmium batteries, and lithium-ion batteries.
What is galvanization?
Galvanization is the process of coating a metal with a layer of zinc to protect it from corrosion. Zinc is more reactive than most metals and is sacrificially corroded in preference to the metal being protected. This prevents the underlying metal from corroding and extends its lifespan.
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