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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⁺?

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

{CaCl}_{2} ⇌ {Ca}^{2 +} + 2 {Cl}^{-} {Ca}^{2 +} + 2 e^{-} \to Ca 2 mol 1 mol (= 40) (reduction of {Ca}^{2 +})

40 g of calcium needs = 2 mol of electrons = 2 Faraday . (∵ 1 mole of e = 1 F)

The balance reaction will

The charge on Ca in CaCl₂

Ca + 2Cl = 0

Cl has –1 charge so that

Ca + 2(–1) = 0

Ca = 2

We have to get 2o g Ca from Ca ²⁺

Number of required moles = mass / molar mass

Molar mass of Ca is 40 g/mol and required mass of Ca is 20 g

Hence number of moles = 20/40 = 0.5 mol

Electricity required to produce 1 mol of calcium = 2 F

The electricity required to produce 0.5 mol of calcium

= 0.5 × 2 F

= 1 F

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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

136. How much electricity in terms of Faraday is required to produce20.0 g of Ca from molten CaCl2?

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