Name the reducing agent in the following reaction : 3MnO2 + 4AL = 3Mn + 2AL2O3
state which is more reactive Mn or AL and why ?
Answers
Answer:
Al is ‘more reactive’ than Mn as it replaces the Mn from its compound .
3MnO2 + 4AL ------> 3Mn + 2AL2O3
Here changes to Mn. The ‘oxidation number’ of Mn in is +4 whereas the oxidation number of Mn is zero. Hence the change in oxidation number occurs from +4 to 0. Overall oxidation number decreases hence it is reduction and is called as oxidizing agent.
On the contrary, the oxidation number of Al is zero and it changes to +3 in . Hence the ‘oxidation number increases’ so it is an oxidation reaction and Al is a reducing agent.
The reducing agent in the following reaction: 3MnO₂ + 4AL → 3Mn + 2AL₂O₃ is AL.
Explanation:
MnO₂ is an oxidizing agent, AL is a reducing agent.
An oxidizing agent, or oxidant, absorbs electrons and is decreased in the event of a chemical reaction. A reducing agent, or a resistant agent, destroys electrons and is oxidized in a chemical reaction. A reducing agent is usually present in one of its lowest potential oxidation states and is known as an electron donor. AL is the reducing agent in the reaction. According to the Reactivity series, Aluminum remains in the Low Reactivity category compared to Manganese. Aluminum is also more reactive than Manganese.
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