In the given unbalanced redox reaction: C r 2 O 7 2 - + C 2 O 4 2 - → H + C r 3 + , C O 2 One mole of the reducing agent is losing how many moles of e⁻?

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In the given unbalanced redox reaction:

$C r_{2} O_{7}^{2 -} + C_{2} O_{4}^{2 -} \overset{H^{+}}{\to} C r^{3 +}, C O_{2}$

One mole of the reducing agent is losing how many moles of e⁻?

Answer:

Solution:

In the given redox reaction, the reducing agent is the oxalate ion, C₂O₄²⁻. its one mole , when converted into CO₂, loses 2 moles of electrons.

$1 C_{2} O_{4}^{2 -} ⟶ 2 C O_{2} + 2 e^{-}$

Stream:JEESubject:ChemistryTopic:Mole ConceptSubtopic:Calculation of mole

⏱ 2mℹ️ Source: QB

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