any device in which electrical energy is converted to chemical energy, or vice versa called an electrolytic cell. Such a cell typically consists of two metallic or electronic conductors (electrodes) held apart from each other and in contact with an electrolyte (q.v.), usually a dissolved or fused ioRead more
any device in which electrical energy is converted to chemical energy, or vice versa called an electrolytic cell. Such a cell typically consists of two metallic or electronic conductors (electrodes) held apart from each other and in contact with an electrolyte (q.v.), usually a dissolved or fused ionic compound.
A Galvanic cell converts chemical energy into electrical energy. An electrolytic cell converts electrical energy into chemical energy. Here, the redox reaction is spontaneous and is responsible for the production of electrical energy.
A Galvanic cell converts chemical energy into electrical energy. An electrolytic cell converts electrical energy into chemical energy. Here, the redox reaction is spontaneous and is responsible for the production of electrical energy.
In electrochemistry, a salt bridge or ion bridge is a laboratory device used to connect the oxidation and reduction half-cells of a galvanic cell (voltaic cell), a type of electrochemical cell. It maintains electrical neutrality within the internal circuit.
In electrochemistry, a salt bridge or ion bridge is a laboratory device used to connect the oxidation and reduction half-cells of a galvanic cell (voltaic cell), a type of electrochemical cell. It maintains electrical neutrality within the internal circuit.
Oxidation–reduction reactions, commonly known as redox reactions. A redox reaction is defined as a reaction in which oxidation and reduction take place simultaneously. These type of reactions that involve the transfer of electrons from one species to another. The species that loses electrons is saidRead more
Oxidation–reduction reactions, commonly known as redox reactions. A redox reaction is defined as a reaction in which oxidation and reduction take place simultaneously. These type of reactions that involve the transfer of electrons from one species to another. The species that loses electrons is said to be oxidized, while the species that gains electrons is said to be reduced.
(i) Cu²⁺ + 2e⁻ ⟶ Cu(s) (reduction half reaction)
(ii) Zn(s) ⟶ Zn²⁺ + 2e⁻ (oxidation half reaction)
What is an electrolytic cell?
any device in which electrical energy is converted to chemical energy, or vice versa called an electrolytic cell. Such a cell typically consists of two metallic or electronic conductors (electrodes) held apart from each other and in contact with an electrolyte (q.v.), usually a dissolved or fused ioRead more
any device in which electrical energy is converted to chemical energy, or vice versa called an electrolytic cell. Such a cell typically consists of two metallic or electronic conductors (electrodes) held apart from each other and in contact with an electrolyte (q.v.), usually a dissolved or fused ionic compound.
See lessWhat is the difference between galvanic cell and electrolytic cell?
A Galvanic cell converts chemical energy into electrical energy. An electrolytic cell converts electrical energy into chemical energy. Here, the redox reaction is spontaneous and is responsible for the production of electrical energy.
A Galvanic cell converts chemical energy into electrical energy. An electrolytic cell converts electrical energy into chemical energy. Here, the redox reaction is spontaneous and is responsible for the production of electrical energy.
See lessWhat is meant by salt bridge?
In electrochemistry, a salt bridge or ion bridge is a laboratory device used to connect the oxidation and reduction half-cells of a galvanic cell (voltaic cell), a type of electrochemical cell. It maintains electrical neutrality within the internal circuit.
In electrochemistry, a salt bridge or ion bridge is a laboratory device used to connect the oxidation and reduction half-cells of a galvanic cell (voltaic cell), a type of electrochemical cell. It maintains electrical neutrality within the internal circuit.
See lessWhy is KCl used in salt bridge?
KCl is used in salt bridge because: (i) It provides equal number of K⁺ and Cl⁻ ions. (ii) KCl as a salt bridge maintains neutrality in the system.
KCl is used in salt bridge because:
See less(i) It provides equal number of K⁺ and Cl⁻ ions.
(ii) KCl as a salt bridge maintains neutrality in the system.
What is redox reaction?
Oxidation–reduction reactions, commonly known as redox reactions. A redox reaction is defined as a reaction in which oxidation and reduction take place simultaneously. These type of reactions that involve the transfer of electrons from one species to another. The species that loses electrons is saidRead more
Oxidation–reduction reactions, commonly known as redox reactions. A redox reaction is defined as a reaction in which oxidation and reduction take place simultaneously. These type of reactions that involve the transfer of electrons from one species to another. The species that loses electrons is said to be oxidized, while the species that gains electrons is said to be reduced.
See less(i) Cu²⁺ + 2e⁻ ⟶ Cu(s) (reduction half reaction)
(ii) Zn(s) ⟶ Zn²⁺ + 2e⁻ (oxidation half reaction)