Identify the oxidizing agent and reducing agent

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In the reaction Sn(s) + NO3- → SnO2(s) + NO(g), tin (Sn) acts as the reducing agent by losing four electrons, while nitrogen (N) in the nitrate ion acts as the oxidizing agent by gaining three electrons. Oxygen remains unchanged in oxidation state at -2 and does not participate in the electron transfer. The identification of the agents is confirmed as correct. Understanding the roles of each element is crucial for balancing redox reactions effectively.
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Homework Statement


Sn(s)+NO3--->SnO2(s)+NO(g)

Homework Equations


The Attempt at a Solution


0 |+5 ,-2| |+4,-2| |+2,-2|
Sn(s)+NO3--->SnO2(s)+NO(g)
Sn lost 4e reducing agent
N gain 3e oxidizing agent
is that right?
What about oxygen?? do i do the same thing?
thanks
 
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The Oxygen is neither gained nor lost electrons. It stays by -2.
and yes I thibk you`re right.
 
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