Complete and balance the following redox equation using the set of smallest whole?number...

Question:

Complete and balance the following redox equation using the set of smallest whole?number coefficients. Now sum the coefficients of all species in the balanced equation. (Remember the coefficients that are equal to one.) The sum of the coefficients is Br2 (aq) + Sb3+(aq) --> Br-(aq) + Sb5+(aq) (acidic solution).

4

12

13

17

none of these

Redox Reaction:

In a redox reaction, the oxidation and reduction take place simultaneously.

To balance the redox reaction it is divided into two parts oxidation half and reduction half after balancing these half equations we add them.

Answer and Explanation: 1

Below is the reaction has been given:

{eq}Br_2 (aq) + Sb^{3+}(aq) \rightarrow Br^-(aq) + Sb^{5+} {/eq}

Oxidation half reaction

{eq}Sb^{3+}(aq) \rightarrow Sb^{5+} {/eq}

Balancing oxidation half-reaction:

{eq}Sb^{3+}(aq) \rightarrow Sb^{5+} + 2e^- {/eq}

Reduction half reaction

{eq}Br_2 \rightarrow 2Br^- {/eq}

Balancing reduction half-reaction:

{eq}Br_2 + 2e^- \rightarrow 2Br^- {/eq}

Adding both the equation we get,

{eq}Br_2 (aq) + Sb^{3+}(aq) \rightarrow 2Br^-(aq) + Sb^{5+} {/eq}

  • The sum of the coefficient is 5, so None of these is the correct option.

Learn more about this topic:

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Balancing Redox Reactions and Identifying Oxidizing and Reducing Agents

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Chapter 10 / Lesson 13
173K

Learn about oxidizing and reducing agents, how to find them, and how to identify them in redox reactions. Learn about the different types of redox reactions and how to identify a redox reaction.


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