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Match the items of Column I and Column II. Column I Column II (i) K (a) I × t (ii) Λm (b) ΛmΛm0 (iii) α (c) Kc (iv) Q (d) G⋅R

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प्रश्न

Match the items of Column I and Column II.

Column I Column II
(i) K (a) I × t
(ii) Λm (b) `Λ_m/Λ_m^0`
(iii) α (c) `K/c`
(iv) Q (d) `G^∗/R`
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उत्तर

Column I Column II
(i) K (d) `G^∗/R`
(ii) Λm (c) `K/c`
(iii) α (b) `Λ_m/Λ_m^0`
(iv) Q (a) I × t
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अध्याय 3: Electrochemistry - Exercises [पृष्ठ ४१]

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एनसीईआरटी एक्झांप्लर Chemistry Exemplar [English] Class 12
अध्याय 3 Electrochemistry
Exercises | Q IV. 53. | पृष्ठ ४१

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At 25°C, the emf of the following electrochemical cell.

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Consider the change in the oxidation state of Bromine corresponding to different emf values as shown in the expression below:

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Then the species undergoing disproportionation is:


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Oxidation-reduction reactions are commonly known as redox reactions. They involve transfer of electrons from one species to another. In a spontaneous reaction, energy is released which can be used to do useful work. The reaction is split into two half-reactions. Two different containers are used and a wire is used to drive the electrons from one side to the other and a Voltaic/Galvanic cell is created. It is an electrochemical cell that uses spontaneous redox reactions to generate electricity. A salt bridge also connects to the half-cells. The reading of the voltmeter gives the cell voltage or cell potential or electromotive force. If \[\ce{E^0_{cell}}\] is positive the reaction is spontaneous and if it is negative the reaction is non-spontaneous and is referred to as electrolytic cell. Electrolysis refers to the decomposition of a substance by an electric current. One mole of electric charge when passed through a cell will discharge half a mole of a divalent metal ion such as Cu2+. This was first formulated by Faraday in the form of laws of electrolysis.
The conductance of material is the property of materials due to which a material allows the flow of ions through itself and thus conducts electricity. Conductivity is represented by k and it depends upon nature and concentration of electrolyte, temperature, etc. A more common term molar conductivity of a solution at a given concentration is conductance of the volume of solution containing one mole of electrolyte kept between two electrodes with the unit area of cross-section and distance of unit length. Limiting molar conductivity of weak electrolytes cannot be obtained graphically.

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Two metal plates or wires through which the current enters and leaves the electrolytic cell.


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