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Electrochemistry

Short Answer Type

131. Write the cell reactions which occur in lead storage battery (i) when the battery is in use and (ii) when the battery is on charging.

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132. The conductivity of 0.20 M solution of KCl at 298 K is 0.0248 s cm^–1. Calculate its molar conductivity.

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133.

How much charge is required for the following reductions:
1 mol of Al³⁺ to Al?

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134.

How much charge is required for the following reductions:
1 mol of Cu²⁺ to Cu?

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135.
How much charge is required for the following reductions:
1 mol of MnO₄^– to Mn²⁺?

{MnO}_{4}^{-} (aq) + 8 H^{+} + 5 e^{-} \to {Mn}^{2 +} (aq) + 6 H_{2} O . 1 mol 5 moles 1 mol

Formula required charge n × F

n = difference of charge on ions

F is constant and equal to 96487 Coulombs

Charge on Mn in MnO4^–

Charge on Oxygen is – 2

Mn + 4O = – 1

Mn +4(–2) = – 1

Mn = +7

So our reaction is

MN ⁷⁺ à Mn ²⁺

n = 7– 2 = 5
Here n= 5

Required charge will = 5 × 96487 Coulombs

= 482435 Coulombs

= 4.82 × 10⁵ Coulombs

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136. How much electricity in terms of Faraday is required to produce
20.0 g of Ca from molten CaCl₂?

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137. How much electricity in terms of Faraday is required to produce
40.0 g of Al from molten Al₂O₃?

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138. How much electricity is required in coulomb for the oxidation of
1 mol of H₂O to O₂ ?

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139. How much electricity is required in coulomb for the oxidation of
1 mol of FeO to Fe₂O₃

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140. A solution of Ni(NO₃)₂ is electrolysed between platinum electrodes using a current of 5 amperes for 20 minutes. What mass of Ni is deposited at the cathode?

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Previous Year Papers

Test Series

Test Yourself

Short Answer Type

135. How much charge is required for the following reductions:1 mol of MnO4– to Mn2+?

135.
How much charge is required for the following reductions:
1 mol of MnO₄^– to Mn²⁺?