Questions in electrochemistry

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During electrolysis of fused aluminium chloride 0.9 gm of aluminium was deposited on the cathode. The volume of chlorine liberated at the anode will be
On passing 3 Ampere of electricity for 50 minutes, 1.8 gram metal deposits. The equivalent mass of metal is
The mass of copper deposited from a solution of $CuS{{O}_{4}}$ by passage of 5 A current for 965 second is (Mol. wt. of Copper = 63.5)
5 Amperes is passed through a solution of zinc sulphate for 40 minutes. Find the amount of zinc deposited at the cathode
In an electroplating experiment $m$ g of silver is deposited, when 4 Amperes of current flows for 2 minutes. The amount (in gms) of silver deposited by 6 Amperes of current flowing for 40 seconds will be
On passing electric current through molten aluminium chloride, 11.2 litre of $Cl_2$ is liberated at NTP at anode. The quantity of aluminium deposited at cathode is (at. wt. of $Al = 27$)
A conducting wire carries a current of $0.965$ Ampere. Rate of flow of electrons per second at a given point is
An electrolytic cell contains a solution of $A{{g}_{2}}S{{O}_{4}}$and have platinum electrodes. A current is passed until 1.6 gm of $O_2$ has been liberated at anode. The amount of silver deposited at cathode would be
A certain quantity of electricity is passed through an aqueous solution of $AgN{{O}_{3}}$ and cupric salt solution connected in series. The amount of Ag deposited is 1.08 gm, the amount of copper deposited is (atomic weight of $Cu = 63.5$; $Ag = 108$)
An electric current is passed through silver voltameter connected to a water voltameter. The cathode of the silver voltameter weighed $0.108 g$ more at the end of the electrolysis. The volume of oxygen evolved at STP is

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