Match each redox reaction in Column I with the mole ratio of oxidizing agent to reducing agent in Column II. Column I Column II A) Mn O 4 − + C 2 O 4 2 − → M n 2 + + C O 2 (acidic) P) 2:5 B) C

Question

Match each redox reaction in Column I with the mole ratio of oxidizing agent to reducing agent in Column II.

Column I	Column II
A) $Mn O_{4}^{-}$ + $C_{2} O_{4}^{2 -}$ $\to$ $M n^{2 +}$ + $C O_{2}$ (acidic)	P) 2:5
B) $C r_{2} O_{7}^{2 -}$ + $F e^{2 +}$ $\to$ $C r^{3 +}$ + $F e^{3 +}$	Q) 1:6
C) $Mn O_{4}^{-}$ + $F e^{2 +}$ $\to$ $M n^{2 +}$ + $F e^{3 +}$	R) 1:5
D) $N O_{3}^{-}$ + Cu $\to$ $NO$ + $C u^{2 +}$ (dilute acid)	S) 2:3

TestHub · Accepted Answer

(A) Mn(+7) → +2 gains 5 e − ; C 2 ​ O 4 2 − ​ loses 2 e − : 2 Mn O 4 − ​ : 5 C 2 ​ O 4 2 − ​ , ratio 2:5 (P). (B) C r 2 ​ O 7 2 − ​ gains 6 e − ; F e 2 + loses 1 e − : ratio 1:6 (Q). (C) Mn O 4 − ​ gains 5 e − ; F e 2 + loses 1 e − : ratio 1:5 (R). (D) N(+5) → NO ( + 2 ) gains 3 e − ; Cu loses 2 e − : 2 N O 3 − ​ : 3 Cu, ratio 2:3 (S).

Chemistry - Redox Reactions Question with Solution | TestHub

Options:

Doubts & Discussion