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Question

Balance the following redox reactions:

Al(s)+H2SO4(aq)Al2(SO4)3(aq)+H2(g)

A
2Al(s)+3H2SO4(aq)Al2(SO4)3(aq)+3H2(g)
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B
5Al(s)+4H2SO4(aq)Al2(SO4)3(aq)+2H2(g)
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C
4Al(s)+H2SO4(aq)Al2(SO4)3(aq)+3H2(g)
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D
5Al(s)+4H2SO4(aq)Al2(SO4)3(aq)+5H2(g)
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Solution

The correct option is A 2Al(s)+3H2SO4(aq)Al2(SO4)3(aq)+3H2(g)
The balanced reaction is as follows:
2Al(s)+3H2SO4(aq)Al2(SO4)3(aq)+3H2(g)
Aluminium is getting oxidized from 0 to +3.
So, there is a factor of 3 before sulphuric acid and hydrogen.
Hydrogen is getting reduced from 1 to 0.
Here, there are 2×1 electrons involved.
Hence, there will be a factor of 2 before Al and aluminium sulphate.
Hence, the correct equation is in option A.

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