Electrochemistr...

In electrolysis of NaCl when Pt electrode is taken then $${ H }_{ 2 }$$ is liberated at the cathode while with Hg cathode it forms sodium amalgam, because:

How long (approximate) should water be electrolysed by passing through $$100$$ amperes current so that the oxygen released can completely burn $$27.66\ g$$ of diborane?
[Atomic weight of $$B=10.8\ u$$]

In the electrolysis of $$AgNO_3$$ solution 0.7 g of Ag is deposited after a certain period of time. Calculate the quantity of electricity required in coulomb. Molar mass of Ag is $$107.9 g mol^{-1}$$.

Based on the cell notation for spontaneous reaction, at the anode:
$$Ag(s)|AgCl(s)|{ Cl }^{ - }(aq)\parallel { Br }^{ - }(aq)|{ Br }_{ 2 }(I)|C(s)$$

$$10800\ C$$ of electricity through the electrolyte deposited $$2.977\ g$$ of metal with atmic mass $$106.4\ g\ mol^{-1}$$. The charge on the metal cation is:

$$Al_2O_3$$ is reduced by electrolysis at low potentials and high currents. If $$4.0\times 10^4$$ amperes of current is passed through molten $$Al_2O_3$$ for $$6$$ hours, what mass of aluminium is produced? 

If a $$100 \; mL$$ solution of $$0.1M$$. $$HBr$$ is titrated using a very concentrated solution of $$NaOH$$, then the conductivity (specific conductance) of this solution at the equivalence point will be:

The number of coulombs necessary to deposit 1 g of potassium metal (molar mass $$39 g mol^{-1}$$) from $$K^+ ions$$ is:

When $$9.65$$ ampere current was passed for $$1.0$$ hour into nitrobenzene in acidic medium, the amount of p-aminophenol produced is:

The charge required to deposit $$40.5 \,g$$ of $$Al$$ (atomic mass $$= 27.0 \,g$$) from the fused $$Al_2(SO_4)_3$$ is: