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Electrochemistry

Long Answer Type

111. What is the Nernst equation for the Potential of an electrode? Can Nernst equation be applied to the cell relation ? Apply this equation to a general reaction.

aA + bB \to cC + dD

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112. Explain Kohlrausch’s law of independent migration of ions. Mention one application of Kohlrausch’s law.

900 Views

Short Answer Type

113. How does molar conductivity vary with concentration for (i) weak electrolyte and for (ii) strong electolyte? Give reasons for these variations.

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114. State and explain Faraday's law of electrolysis?

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Long Answer Type

115. State and explain Faraday's law of electrolysis?

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116. Show that the electrical work obtainable from a galvanic cell is given by the expression.

∆ G ° = - nFE °_{cell}

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Short Answer Type

117. What are fuel cells? Write the reaction of a oxygen hydrogen fuel cell.

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118.

What is a mercury cell? Give the electrode reactions?

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119. What is the effect of change in (a) concentration, (b) temperature on the electrode potential of a given half-cell?

For a half-cell in which the electrode reaction is,

M^{n +} + {ne}^{-} = M

The Nernst equation is

E = E °_{M^{n +} / M} - \frac{2.303 RT}{nF} \log \frac{1}{[M^{n +}]} = E °_{M^{n +} / M} + \frac{2.303 RT}{nF} \log [M^{n +}]

From the equation, E ∝ T and E ∝ [Mⁿ⁺]
(a) When the concentration of Mⁿ⁺ increases, the half-cell potential increases and vice-versa.
(b) When temperature increases, the half-cell potential also increases.

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120. Iron does not rust even if the zinc coating is broken in a galvanised iron pipe but, rusting occurs much faster if the tin coating over iron is broken. Explain?

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