Home
Class 12
CHEMISTRY
Aluminium oxide may be electrolysed at 1...

Aluminium oxide may be electrolysed at `1000^(@)C` to furnish aluminium metal (Atomic mass=27u, 1F=96500C). The cathode reaction is
`Al^(3+)+3e^(-)toAl^(0)`
To prepare 5.12 kg of aluminium metal by this method would require

A

`5.49xx10^(4)C` of electricity

B

`5.49xx10^(1)C` of electricity

C

`5.49xx10^(7)C` of electricity

D

`1.83xx10^(7)C` of electricity.

Text Solution

Verified by Experts

The correct Answer is:
C
`Al^(3+)+3e^(-)rarrAl`
`3xx96500 27g`
To produce 27g of Al, electricity required
`=3xx96500C`
`therefore` To produce 5.12kg of Al, electricity required
`=(3xx96500)/(27)xx5.12xx10^(3)C`
`=5489.78xx10^(3)C=5.49xx10^(7) C`
Promotional Banner

Similar Questions

Explore conceptually related problems

Aluminium oxide may be electrolysed at 1000^(@) C to furnish aluminium metal (Atomic mass = 27 amu, 1 Faraday = 96500 Coulomb). The cathode reaction is Al^(3+) + 3e^(-) rightarrow Al . To prepare 5.12 kg of aluminium metal by this method would require:

When aluminium oxide (Al_(2)O_(3)) is electrolysed for the production of aluminium metal. For a given quantity of electricty, the number of moles of aluminium obtained if the volume of O_(2) gas obtained is 201.6 litre measured at NTP, is

In the commercial preparation of aluminum,aluminum oxide (Al_2O_3) is electrolysed at 1000^(@) C. How many coulombs of electricity are required to give 54kg of aluminum ? Assume following reaction takes place at cathode: Al^(3+)+3e^- \to Al

Chemical reactions involve interaction of atoms and molecules. A large number of atoms and molecules (approximately 6.022 xx 10^(23) ) are present in a few grams of any chemical compound varying with their atomic/molecular masses. To handle such a large number conveniently, the mole concept was introduced. This concept has implications in diverse areas such as analytical chemistry, biochemistry, electrochemistry adn radiochemistry. The following examples illustrate a typical case involving chemical/electrochemical reaction which requires a clear understanding of mole concept. A 4.0 molar aqueous solution of NaCl is prepared and 500 mL of the solution is electrolysed. This lead to the evolution of chlorine gas at one of electrodes (atomis mass : Na = 23 , Hg = 200 , 1F = 96500 C) If the cathode is a Hg electrode, the maximum weight (g) of amalgam formed from the solution is :

The density of aluminium (atomic mass = 27) is 2700 kg m^(-3) . If Al has feestructure, calculate its atomic radius.

Calculate the amount of electricity required to deposite 0.9 g of aluminium by electrolysis of a salt containing its ion, if the electrode reaction is Al^(3+)+3e^(-)rarrAl , (atomic mass of Al =27, 1F=96500C )

Despite the fact that aluminium is a reactive metal, it is a stable in air as well as in water. This is due to the formation of thin layer of oxide on the surface of aluminium metal which makes it passive for further attack. The layer is so useful, that in industry, it is purposely deposited by an electrolytic process called anodising. Reaction of aluminium with oxygen is highly exothermic and is called thermite reaction. 2Al_((s)) +(3)/(2) O_(2(g)) rarr Al_(2)O_(3(s)) Delta_(f) H^(Ө) = -1670 kJmol^-1 This reaction finds application for welding of metal and in the metallurgical extraction of many metals from their oxides. The limitation is that to start the reaction, high temperature is required for which an ignition mixture is required. Aluminium becomes passive in :

Despite the fact that aluminium is a reactive metal, it is a stable in air as well as in water. This is due to the formation of thin layer of oxide on the surface of aluminium metal which makes it passive for further attack. The layer is so useful, that in industry, it is purposely deposited by an electrolytic process called anodising. Reaction of aluminium with oxygen is highly exothermic and is called thermite reaction. 2Al_((s)) +(3)/(2) O_(2(g)) rarr Al_(2)O_(3(s)) Delta_(f) H^(Ө) = -1670 kJmol^-1 This reaction finds application for welding of metal and in the metallurgical extraction of many metals from their oxides. The limitation is that to start the reaction, high temperature is required for which an ignition mixture is required. Anodised aluminium is.

Despite the fact that aluminium is a reactive metal, it is a stable in air as well as in water. This is due to the formation of thin layer of oxide on the surface of aluminium metal which makes it passive for further attack. The layer is so useful, that in industry, it is purposely deposited by an electrolytic process called anodising. Reaction of aluminium with oxygen is highly exothermic and is called thermite reaction. 2Al_((s)) +(3)/(2) O_(2(g)) rarr Al_(2)O_(3(s)) Delta_(f) H^(Ө) = -1670 kJmol^-1 This reaction finds application for welding of metal and in the metallurgical extraction of many metals from their oxides. The limitation is that to start the reaction, high temperature is required for which an ignition mixture is required. Which of the following metals cannot be extracted by using Al as a reducing agent ?

Despite the fact that aluminium is a reactive metal, it is a stable in air as well as in water. This is due to the formation of thin layer of oxide on the surface of aluminium metal which makes it passive for further attack. The layer is so useful, that in industry, it is purposely deposited by an electrolytic process called anodising. Reaction of aluminium with oxygen is highly exothermic and is called thermite reaction. 2Al_((s)) +(3)/(2) O_(2(g)) rarr Al_(2)O_(3(s)) Delta_(f) H^(Ө) = -1670 kJmol^-1 This reaction finds application for welding of metal and in the metallurgical extraction of many metals from their oxides. The limitation is that to start the reaction, high temperature is required for which an ignition mixture is required. Anodising can be done by elecrolysing dil H_(2)SO_(4) with Al as anode. This results in :