Home
Class 12
PHYSICS
A study potential difference of 1.62 V i...

A study potential difference of 1.62 V is maintained across two Pt electrodes placed in a solution of `CuCl_(2)` . At the end of 600s, the mass of copper deposited on the cathode is measured to be 5.92 g. The back emf of the voltameter is given to be 1.34 V. Estimate the resistance of voltameter. Faraday constant =96500 C `mol^(-1)`, relative atomic mass of copper =63.5.

Promotional Banner

Similar Questions

Explore conceptually related problems

A steady e,.m .f of 1.72 is maintaied across two platinum electrodes placed in a solution of CuCl_(2) At the end o f510 s, the mass of copper deposit is 5.1 f the back e,.m f of votameter is given to be 1.527 V Calculate the resistance of the voltmeter [Faradays constant =96500 C "mole" ^(-1) , Atomic mass of copper =63.5 ]

It is desired to deposit 0.254 kg of copper on the cathode of a copper voltameter . How long will it take to deposit this amount if a steady current of 100 A is maintained . Use the known value of Faraday constant . Relative atomic mass of copper is 63.5 .

In copper plateing experiment 6.35 g of copper is deposit in one and a half hours An ammeter connected in series records a currect of 3.5 A Calculate the error in ammeter reading . [F=96500 C mol^(-1) ,"gram atomic mass of copper "=63.5 g]

A solution of CuSO_(4) is electrolysed for 10 minutes with a current of 1.7 amperes. What is the mass of copper deposited at the cathode? (Molar mass of Cu= 63.5g/mol).

A steady current of 10.0 A is maintained in a copper voltameter . Calculate the time required to deposit 2.5 g of copper . Relative atomic mass of copper = 63.5 g .

A solution of CuSO_(4) is electroysed for 10 minutes with a current of 1.5 amperes. What is the mass of copper deposited at the cathode ? (Molar mass of Cu=63.5 g//mol)