Answer:
The balanced net ionic equation is as follows:
CrO₄²- (aq) + 3 N₂O (g) + 2 H+ (aq) ----> Cr³+ (aq) + 6 NO (g) + H₂O (l)
The oxidizing agent is CrO₄²- as Cr⁶+ in CrO₄²- is reduced to Cr³+.
The reducing agent is N₂O as the nitrogen (i) is oxidized to nitrogen (ii).
Step-by-step explanation:
The skeleton equation is given as follows:
CrO₄²- (aq) + N₂O(g)+ H+(aq) + OH-(aq) + H2O(l) ----> Cr³+(aq) + NO(g) + H+(aq) + OH-(aq) + H₂O(l)
The balanced net ionic equation with the spectator ions removed is as follows:
CrO₄²- (aq) + 3 N₂O (g) + 2 H+ (aq) ----> Cr³+ (aq) + 6 NO (g) + H₂O (l)
In a redox reaction, oxidizing agents are reduced while reducing agents are oxidized.
The oxidizing agent is CrO₄²- as Cr⁶+ in CrO₄²- is reduced to Cr³+.
One mole of CrO₄²- accepts three moles of electrons from three moles of N₂O to become reduced to 1 mole of Cr³+.
The reducing agent is N₂O as the nitrogen (i) is oxidized to nitrogen (ii).
Three moles of N₂O will each donate one mole of electrons to one mole of CrO₄²- to become oxidized to nitrogen (ii) oxide.
Hydrogen ions and a water molecule is added to the left-hand side and right-hand side of the equation respectively, in order to balance the number of oxygen atoms in the equation of the reaction.