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241. How is an electrode potential measured?

The electrode potential measures the tendency of electrons to flow away from or towards a redox equilibrium. They are always measuredwith respect to the standard hydrogen electrode (which is assigned a value of zero volts).

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242. Write a Nernst equation for the half-cell reaction: Mⁿ⁺(aq) + ne^– → M(s)

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243. Write the Nernst equation for a galvanic cell corresponding to the reaction:

Zn (s) + {Cu}^{2 +} (aq) \to Zn (aq) + Cu (s)

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244.

Electrolysis of molten NaCl gives sodium at cathode while aqueous NaCl gives H₂ gas at cathode.

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245. What is dry cell? Explain its working.

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246. Draw curves to show how the molar conductance of strong electrolytes varies with dilutions.

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247. How the Kohlrausch’s law is used to determine the degree of ionization of weak electrolyte?

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248. For the cell Zn/Zn²⁺ (aq) || Cu²⁺(aq) | Cu, derive the relation between E°_cell and K_c at 298 k.

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249. For the standard cell, Cu(s) | Cu²+(aq) || Ag⁺ (aq) | Ag(s)
Given: E° _Cu²⁺/Cu = 0.34V, E° = 0.80V
(a) Identify cathode and anode as the current is drawn through the cell.
(b) Write the reactions taking place at the electrodes.
(c) Calculate the standard cell potential.

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