Assertion :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 $S n (s)$ . Reason: In balancing half reaction, $S_{2} O_{3}^{2 -} \to S (s)$ , the number of electrons added on the left is 4.

Both Assertion and Reason are correct and Reason is the correct explanation for Assertion

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Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion

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Assertion is correct but Reason is incorrect

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Assertion is incorrect but Reason is correct

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Solution

The correct option is B Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
Assertion:
$8 H^{+} + 4 N O_{3}^{-} + 6 C l^{-} + S n_{(s)} \to S n C l_{6}^{2 -} + 4 N O_{2} + 4 H_{2} O$
As $S n (s)$ in left side , has O.S. to be $0$ , then as in $S n C l_{6}^{2 -}$ , $S n$ has $+ 4$ .

Hence reducing agent is that species which undergo oxidation or increases O.S. which is here $S n (s)$ , Hence assertion is correct.

Reason: $S_{2} O_{3}^{2 -} \to 2 S_{(s)}$
As in $S_{2} O_{3}^{2 -}$ the oxidation state of $S$ is $+ 2$ , hence it must add $2$ electron to get per $S (s)$ atom, hence total electron to be added is $4$ .

Although reason is a correct statement, it is not the correct explanation to assertion, only the explanation given for the solution is the reason.

Hence Option B.

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Choose the correct option.

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Assertion :In the redox reaction, 8H+(aq)+4NO−3+6Cl−+Sn(s)→SnCl2−6+4NO2+4H2O, the reducing agent is Sn(s). Reason: In balancing half reaction, S2O2−3→S(s), the number of electrons added on the left is 4.

Assertion :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 $S n (s)$ . Reason: In balancing half reaction, $S_{2} O_{3}^{2 -} \to S (s)$ , the number of electrons added on the left is 4.