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Electrochemical Cell and Gibbs Energy of Reaction Video Lecture - JEE
FAQs on Electrochemical Cell and Gibbs Energy of Reaction Video Lecture - JEE
| 1. What is an electrochemical cell? |  |
Ans. An electrochemical cell is a device that converts chemical energy into electrical energy or vice versa. It consists of two half-cells, each containing an electrode and an electrolyte solution. The electrodes are connected by a conducting wire, and the electrolytes allow the transfer of ions between the electrodes. This transfer of ions leads to the flow of electrons, creating an electric current.
| 2. How does an electrochemical cell work? | |
Ans. An electrochemical cell works by harnessing the redox (reduction-oxidation) reactions occurring in the half-cells. In the oxidation half-cell, the electrode loses electrons and undergoes oxidation, while in the reduction half-cell, the electrode gains electrons and undergoes reduction. The flow of electrons from the oxidation half-cell to the reduction half-cell creates an electric current. The reactions at the electrodes are balanced by the movement of ions through the electrolyte, maintaining electrical neutrality.
| 3. What is the significance of Gibbs energy of reaction in electrochemical cells? | |
Ans. The Gibbs energy of reaction, also known as the free energy change (ΔG), is a crucial parameter in electrochemical cells. It determines the spontaneity and feasibility of the redox reaction occurring in the cell. If ΔG is negative, the reaction is spontaneous, and the cell can produce electrical energy. If ΔG is positive, the reaction is non-spontaneous, and an external electrical energy supply is required to drive the reaction. If ΔG is zero, the reaction is at equilibrium, and no net energy is produced.
| 4. How is the Gibbs energy of reaction related to the cell potential? | |
Ans. The Gibbs energy of reaction (ΔG) is directly related to the cell potential (Ecell) through the equation ΔG = -nFEcell, where n is the number of moles of electrons transferred and F is the Faraday constant. This equation shows that the cell potential is a measure of the energy available from the redox reaction. If Ecell is positive, ΔG will be negative, indicating a spontaneous reaction. Conversely, if Ecell is negative, ΔG will be positive, indicating a non-spontaneous reaction.
| 5. How can the Gibbs energy of reaction be used to predict the feasibility of a redox reaction? | |
Ans. The Gibbs energy of reaction (ΔG) can be used to determine whether a redox reaction is thermodynamically favorable or not. If ΔG is negative, the reaction is spontaneous and will proceed in the forward direction. If ΔG is positive, the reaction is non-spontaneous, and it will not occur without the input of external energy. If ΔG is zero, the reaction is at equilibrium, and there will be no net change in the concentrations of reactants and products. By comparing the ΔG value to zero, one can predict whether a reaction will occur spontaneously or not.
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