A steady current of 5 A is maintained for 45 minutes. During this time it deposits 4.572 g of zinc at the cathode of voltameter. Electrochemical equivalent of zinc is:
3.387×10−4kg/C
3.387×10−4g/C
3.384×10−4kg/C
3.384×10−3kg/C
A
3.387×10−4kg/C
B
3.384×10−4kg/C
C
3.384×10−3kg/C
D
3.387×10−4g/C
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Solution
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The electrochemical equivalent of a chemical element is the mass of that element (in grams) transported by 1 coulomb of electricity. The mass of a substance liberated or deposited at an electrode during electrolysis is directly proportional to the quantity of charge passed through the electrolyte.
A steady current of 5 A is maintained for 45 minutes. During this time it deposits 4.572 g of zinc at the cathode of voltameter. Electrochemical equivalent of zinc is:
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Q2
A copper voltameter is connected in series with a coil of resistance 10Ω. When a steady current is passed through the circuit, 0.297g of copper is found to be deposited at the cathode in 15min. The electrochemical equivalent of copper is 3.3×10−7kgC−. Heat liberated in the coil is:
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Q3
A steady current of 1.5A flows through a copper voltameter for 10 min. If the electrochemical equivalent of copper is 30×10−5gC−1, the mass of copper deposited on the electrode will be
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Q4
Copper and silver voltameter are connected in series and an electric current is passed through them for sometime. It is observed that 14g of copper is deposited. Then, calculate the mass of silver deposited.
Given: Electrochemical equivalent of copper =3.2×10−7gC−1 Electrochemical equivalent of silver =1.2×10−6gC−1
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Q5
What is the mass of silver deposited on the passage of 2 A current during the electrolysis of silver? Electrochemical equivalent of silver = 1.18×10−3gmC−1