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Electrochemistry

Short Answer Type

61. What are the units of Λ?

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62. Write the Nernst equation for the following cell:
Pt, Cl₂ (1 atm)/2Cl^– (1 M)

Answer:

E = E ° + \frac{0.059}{2} \log \frac{[{Cl}_{2}]}{{[{Cl}^{-}]}^{2}} = E ° + \frac{0.059}{2} \log \frac{1}{(1)^{2}} .

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63. How does cell constant changes with the concentration of the solution in the conductivity cell.

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64. What are conductors?

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65. What are electrolytes?

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66. How many Faradays of electricity are required to liberate 2 moles of hydrogen gas in electrolysis of solution?

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67. What is meant by Faraday constant?

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68. What is the relation between E_cell of hydrogen electrode and pH of the solution, when this half cell is connected with normal hydrogen electrode (NHE)?

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69. What does the standard electrode potential of a metal being negative (E_Zn2+/Zn = -0.763 V) indicate?

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70. Arrange the following metals in the order in which they displace each other from the solution of their salts Al, Cu, Fe, Mg and Zn.

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Previous Year Papers

Test Series

Test Yourself

Short Answer Type

62. Write the Nernst equation for the following cell:Pt, Cl2 (1 atm)/2Cl– (1 M)

62. Write the Nernst equation for the following cell:
Pt, Cl₂ (1 atm)/2Cl^– (1 M)