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Ch.20 - Electrochemistry
All textbooksBrown 15th EditionCh.20 - ElectrochemistryProblem 19b
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Chapter 20, Problem 19b

Indicate whether the following balanced equations involve oxidation–reduction. If they do, identify the elements that undergo changes in oxidation number. (b) NaI(aq) + 3 HOCl(aq) → NaIO3(aq) + 3 HCl(aq)

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Determine the oxidation states of each element in the reactants and products.
For NaI, Na is in the +1 oxidation state and I is in the -1 oxidation state.
For HOCl, H is in the +1 oxidation state, O is in the -2 oxidation state, and Cl is in the +1 oxidation state.
For NaIO_3, Na is in the +1 oxidation state, I is in the +5 oxidation state, and O is in the -2 oxidation state.
For HCl, H is in the +1 oxidation state and Cl is in the -1 oxidation state.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Oxidation-Reduction Reactions

Oxidation-reduction (redox) reactions involve the transfer of electrons between substances, resulting in changes in oxidation states. In these reactions, oxidation refers to the loss of electrons, while reduction refers to the gain of electrons. Identifying whether a reaction is a redox process requires analyzing the oxidation states of the elements involved before and after the reaction.
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Oxidation States

Oxidation states (or oxidation numbers) are assigned to elements in a compound to indicate their degree of oxidation or reduction. The oxidation state of an element can change during a chemical reaction, which is crucial for identifying redox processes. Common rules for determining oxidation states include that the oxidation state of an element in its elemental form is zero, and for monoatomic ions, it is equal to the charge of the ion.
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Balancing Chemical Equations

Balancing chemical equations ensures that the number of atoms for each element is the same on both sides of the equation, reflecting the conservation of mass. In redox reactions, balancing often involves ensuring that both the number of electrons lost in oxidation and gained in reduction are equal. This process may require adjusting coefficients in front of compounds to achieve balance while maintaining the correct stoichiometry.
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Textbook Question

For each of the following balanced oxidation–reduction reactions, (i) identify the oxidation numbers for all the elements in the reactants and products and (ii) state the total number of electrons transferred in each reaction. (b) 2 Hg2+(aq) + N2H4(aq) → 2 Hg(l) + N2(g) + 4 H+(aq)

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Textbook Question

For each of the following balanced oxidation–reduction reactions, (i) identify the oxidation numbers for all the elements in the reactants and products and (ii) state the total number of electrons transferred in each reaction. (a) 2 MnO4-(aq) + 3 S2-(aq + 4 H2O(l) → 3 S(s) + 2 MnO2(s) + 8 OH-(aq)

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Textbook Question

Indicate whether the following balanced equations involve oxidation–reduction. If they do, identify the elements that undergo changes in oxidation number. (a) PBr3(l) + 3 H2O(l) → H3PO3(aq) + 3 HBr(aq)

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Textbook Question

Indicate whether the following balanced equations involve oxidation–reduction. If they do, identify the elements that undergo changes in oxidation number. (a) 2 AgNO3(aq) + CoCl2(aq) → 2 AgCl(s) + Co(NO3)2(aq)

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Textbook Question

At 900 °C, titanium tetrachloride vapor reacts with molten magnesium metal to form solid titanium metal and molten magnesium chloride. (a) Write a balanced equation for this reaction.

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Textbook Question

Hydrazine 1N2H42 and dinitrogen tetroxide 1N2O42 form a self-igniting mixture that has been used as a rocket propellant. The reaction products are N2 and H2O. (c) Which substance serves as the reducing agent and which as the oxidizing agent?

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