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Electrochemistry

Short Answer Type

181. Write the Nernst equation and emf of the following cells at 298 k.
Mg(s) | Mg²⁺ (0.001 M) || Cu²⁺ (0.0001 M) | Cu(s)

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182. Write the Nernst equation and emf of the following cells at 298 k.
Fe(s) | Fe²⁺ (0.001 M) || H⁺ (1M) | H₂ (g) (1 bar) | Pt(s)

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183. Write the Nernst equation and emf of the following cells at 298 k.
Sn(s) | Sn²⁺ (0.050 M) || H⁺(0.020 M) H₂(g) (1bar) Pt (s)

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184. Write the Nernst equation and emf of the following cells at 298 k.
Pt(s) | Br₂ (l) | Br^– (0.010 M) || H⁺ (0.030 M) | + H₂(g) (1 bar) | Pt(s).

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185. What is corrosion? What are the factors which affect corrosion?

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186. CO₂ is always present in natural water. Explain its effect (increases, stops or no effect) on rusting of iron.

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187. Rusting of iron is quicker in saline water than in ordinary water. Explain.

Saline water contains greater number of irons (dissolved salts, NaCl) than ordinary water and therefore electro-chemical reaction is quicker with saline water than when ordinary water is present. This increases rate of corrosion of metal.

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188. We can use aluminium in place of zinc for cathodic protection of rusting. Comment.

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189. How is cathodic protection of Iron different from its galvanisation?

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Long Answer Type

190. Define conductivity and molar conductivity for the solution of an electrolyte. Discuss their variaion with concentration.

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