Statement 1: In the redox reaction 8H+ (aq) +4 NO-3 +6Cl-+Sn(s) → snCl2-6 +4NO2 +4H2O, the reducing agent is Sn(s). Statement 2: In balancing half-reaction, S2O2-3 →S(s), the number of electrons added on the left is 4.

Question

Statement 1: In the redox reaction 8H+ (aq) +4 NO-3 +6Cl-+Sn(s) → snCl2-6 +4NO2 +4H2O, the reducing agent is Sn(s). Statement 2: In balancing half-reaction, S2O2-3 →S(s), the number of electrons added on the left is 4. (A) If both Statement 1 and Statement 2 are true and the statement 2 is the correct explanation of the statement 1. (B) Ifboth Statement 1 and Statement 2 are true but statement 2 is not the correct explanation of the statement 1. (C) If Statement 1 is true but Statement 2 is false. (D) If Statement 1 is false but Statement 2 is true.

Tardigrade Admin · Accepted Answer

Sn (0 → + 4) It undergoes oxidation, so it is the reducing agent S2O2-3+6H++4e- → 2S +3H2O

Q. Statement 1: In the redox reaction $8 H^{+} (a q) + 4 N O_{3}^{-} + 6 C l^{-} + S n (s) \to s n C l_{6}^{2 -} + 4 N O_{2} + 4 H_{2} O,$ the reducing agent is Sn(s).
Statement 2: In balancing half-reaction, $S_{2} O_{3}^{2 -} \to$ S(s), the number of electrons added on the left is 4.

If both Statement 1 and Statement 2 are true and the statement 2 is the correct explanation of the statement 1.

Ifboth Statement 1 and Statement 2 are true but statement 2 is not the correct explanation of the statement 1.

If Statement 1 is true but Statement 2 is false.

If Statement 1 is false but Statement 2 is true.

Sn $(0 \to + 4)$
It undergoes oxidation, so it is the reducing agent
$S_{2} O_{3}^{2 -} + 6 H^{+} + 4 e^{-} \to 2 S + 3 H_{2} O$

Q. Statement 1: In the redox reaction 8H+(aq)+4NO3−​+6Cl−+Sn(s)→snCl62−​+4NO2​+4H2​O, the reducing agent is Sn(s). Statement 2: In balancing half-reaction, S2​O32−​→S(s), the number of electrons added on the left is 4.