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Solution: Use the half-reaction method to balance each redox reaction occurring in

Chapter 16, Problem 67P

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QUESTION:

Use the half-reaction method to balance each redox reaction occurring in acidic aqueous solution.

(a) \(\mathrm{ClO}_{4}^{~-}(a q)+\mathrm{Cl}^{-}(a q) \longrightarrow \mathrm{ClO}_{3}^{~-}(a q)+\mathrm{Cl}_{2}(g)\)

(b) \(\mathrm{MnO}_{4}^{~-}(a q)+\mathrm{Al}(s) \longrightarrow \mathrm{Mn}^{2+}(a q)+\mathrm{Al}^{3+}(a q) \)

(c) \(\mathrm{Br}_{2}(a q)+\mathrm{Sn}(s) \longrightarrow \mathrm{Sn}^{2+}(a q)+\mathrm{Br}^{-}(a q)\)

Equation Transcription:

Text Transcription:

ClO_4^-(aq)+Cl-(aq) rightarrow ClO_3-(aq)+Cl2(g)

MnO_4^-(aq)+Al(s) rightarrow  Mn^2+(aq)+Al^3+(aq)

Br_2(aq)+Sn(s) rightarrow  Sn^2+(aq)+Br^-(aq)

Questions & Answers

QUESTION:

Use the half-reaction method to balance each redox reaction occurring in acidic aqueous solution.

(a) \(\mathrm{ClO}_{4}^{~-}(a q)+\mathrm{Cl}^{-}(a q) \longrightarrow \mathrm{ClO}_{3}^{~-}(a q)+\mathrm{Cl}_{2}(g)\)

(b) \(\mathrm{MnO}_{4}^{~-}(a q)+\mathrm{Al}(s) \longrightarrow \mathrm{Mn}^{2+}(a q)+\mathrm{Al}^{3+}(a q) \)

(c) \(\mathrm{Br}_{2}(a q)+\mathrm{Sn}(s) \longrightarrow \mathrm{Sn}^{2+}(a q)+\mathrm{Br}^{-}(a q)\)

Equation Transcription:

Text Transcription:

ClO_4^-(aq)+Cl-(aq) rightarrow ClO_3-(aq)+Cl2(g)

MnO_4^-(aq)+Al(s) rightarrow  Mn^2+(aq)+Al^3+(aq)

Br_2(aq)+Sn(s) rightarrow  Sn^2+(aq)+Br^-(aq)

ANSWER:

Solution 67P: Here, We, are going to balance the equation.

Srep 1:

(a) ClO4 (aq) + Cl (aq) → ClO3 (aq) + Cl2(g)

The balanced chemical equation is

ClO4 (aq) + 2Cl (aq)+2 H+(aq) → ClO3 (aq) + Cl2(g)+ H2O(l)

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