Consider the reaction shown, which occurs in aqueous solutions: NO2^-1 + Al (s) --> NH3 + Al(OH)4^-1 Identify the species reduced: Identify the species oxidized: Identify the reducing agent: Identify the oxidizing agent: The balanced reduction half-reaction: The balanced oxidation half-reaction: Overall balanced redox reaction:
Consider the reaction shown, which occurs in aqueous solutions:
NO2^-1 + Al (s) --> NH3 + Al(OH)4^-1
Identify the species reduced:
Identify the species oxidized:
Identify the reducing agent:
Identify the oxidizing agent:
The balanced reduction half-reaction:
The balanced oxidation half-
Overall balanced redox reaction:
NO2-1 + Al (s) --> NH3 + Al(OH)4-1
the species reduced: NO2-1 ( NO2-1 ==> NH3 , Nitogen reduced as oxidation state decreases from +3 to -3 )
the species oxidized: Al ( Al ==> Al(OH)4-1 , Aluminium oxidised as oxidation state increases from 0 to +3 )
the reducing agent: a substance that has the ability to reduce other substances — in other words to donate/ loose their electrons .
Reducing agent =Al
in given reaction Al looses electron and gets converted into Al+3 i.e. (Al(OH)4-1
the oxidizing agent: a substance that has the ability to oxidize other substances — in other words to accept/ gains their electrons .
Oxidising agent = NO2-1
In given reaction N of NO2-1 in +3 oxidation state , gains 6 e and gets reduced to NH3 in -3 oxidation state
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