An electrolysis reaction is :

In electrolytic cells ...

Electroplating is used to ...

The electrical energy required to produce one kilogram of metal in an electrolytic cell ...

48000 coulombs of charge are required to deposit one-sixth of a mole of a metal. The metal is most likely to be ...

Some metals can only be extracted electrolytically from molten electrolytes. Whether a molten electrolyte is required is determined by ...

The overall equation for an electrolytic cell is:
2H2O(l) + 2Br−(aq) --> Br2(l) + H2(g) + 2OH−(aq)
While this reaction is occurring ...

An electroplating bath is used to plate a uniform layer of silver metal of thickness 0.100 mm onto an object of total surface area 300 cm2. Given that the density of silver is 10.5 g cm^−3, the length of time a current of 2.00 A would need to be passed through the cell to plate the object would be close to ...

The number 96500 is used in many electrolysis calculations.
This number is ...

A current of 1.85 A was passed through a solution containing X2+(aq) ions for precisely 5.00 minutes. 0.169 g of metallic X was deposited on the inert platinum cathode over this time. Metal X is most likely to be ...

Iron can be galvanised (coated with zinc) using an electrolytic process. The maximum mass of zinc which could be deposited on a corrugated iron cathode in 2 hours using a current of 500 amperes would be ...

During the production of aluminium using the Hall-Heroult electrolytic cell, both the anode and cathode are made of carbon, but the carbon only takes part in the reaction at one electrode. Which of the following correctly identifies the reactive carbon electrode, and the product produced at it during the electrolysis?

When determining Avogadro's constant using the electrolysis of a nickel chloride solution, which of the following values is not required?

The products formed at the inert electrodes during the electrolysis of a 1.0 M magnesium iodide solution are ...

In an electroplating cell, a metal ring was to be electroplated with silver. A current of 0.300 A was used to deposit 6.50 mg of silver onto the ring from a silver nitrate solution. The time required to electroplate the ring with silver was close to

When the electrochemical series is used to predict the products of an electrolytic cell reaction ...

The product that would be formed at the graphite anode during the electrolysis of a concentrated aqueous solution of potassium chloride would be ...