Hello,

Here is the answer :-

• Oxidation-Reduction Process : In a redox reaction, the reducing agent donates electrons and is oxidized, while the oxidizing agent accepts electrons and is reduced.

• Excess Reducing Agent : When the reducing agent is in excess, more electrons are donated, leading to a greater reduction of the oxidizing agent, forming a compound with a lower oxidation state.

• Excess Oxidizing Agent : When the oxidizing agent is in excess, it accepts more electrons, leading to the oxidation of the reducing agent and the formation of a compound with a higher oxidation state.

Hope it helps !

Hello Antima,

The statement can be justified as follows:

1. Reduction and Oxidation Process : In a redox reaction, the oxidizing agent gains electrons and undergoes reduction , while the reducing agent loses electrons and undergoes oxidation . When the oxidizing agent is in excess, it will accept more electrons, leading to the formation of a compound in a higher oxidation state (since the oxidizing agent itself is getting reduced).
   
   

2. Excess Reducing Agent : If the reducing agent is in excess, it will provide more electrons to the reaction, causing the oxidizing agent to be reduced to a lower oxidation state. In this case, the compound formed will have a lower oxidation state as the excess reducing agent continues to donate electrons, driving the reduction process.
   
   

3. Equilibrium and Electron Transfer : The oxidation states of the products depend on the availability of electrons for transfer. When the reducing agent is in excess, there is a surplus of electrons for the oxidizing agent to accept, leading to a product with a lower oxidation state. Conversely, if the oxidizing agent is in excess, there are more opportunities for electron acceptance, resulting in a higher oxidation state in the product.
   
   

   
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