Textbook Question
When the nickel–zinc battery, used in digital cameras, is recharged, the following cell reaction occurs: (a) How many grams of zinc are formed when 3.35 x 10-2 g of Ni(OH)2 are consumed?
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Ch.19 - Electrochemistry
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Chapter 19, Problem 150a
Chlorine can be prepared in the laboratory by the reaction of hydrochloric acid and potassium permanganate. (a) Use data in Appendix D to write a balanced equation for the reaction. The reduction product is Mn2+.
Verified step by step guidance1
Identify the reactants and products: Hydrochloric acid (HCl) and potassium permanganate (KMnO4) react to produce chlorine gas (Cl2), manganese(II) ions (Mn2+), and other products.
Write the unbalanced chemical equation: \( \text{HCl} + \text{KMnO}_4 \rightarrow \text{Cl}_2 + \text{Mn}^{2+} + \text{KCl} + \text{H}_2\text{O} \).
Balance the atoms in the equation starting with the manganese (Mn) atoms: Ensure that the number of Mn atoms on both sides of the equation is equal.
Balance the chlorine (Cl) atoms: Since Cl appears in both HCl and Cl2, adjust the coefficients to balance the Cl atoms.
Balance the remaining atoms (H, O, and K) by adjusting the coefficients of HCl, H2O, and KCl, ensuring that the number of each type of atom is equal on both sides of the equation.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Balancing Chemical Equations
Balancing chemical equations involves ensuring that the number of atoms for each element is the same on both sides of the equation. This is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. To balance an equation, coefficients are adjusted in front of the chemical formulas to achieve equal atom counts.
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Balancing Chemical Equations
Redox Reactions
Redox reactions, or reduction-oxidation reactions, involve the transfer of electrons between species. In these reactions, one substance is oxidized (loses electrons) while another is reduced (gains electrons). Understanding the oxidation states of the elements involved is crucial for identifying which species undergo reduction and oxidation during the reaction.
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Oxidation States
Oxidation states (or oxidation numbers) are assigned to atoms in a compound to indicate their degree of oxidation or reduction. They help in tracking electron transfer in redox reactions. For example, in the reaction between hydrochloric acid and potassium permanganate, the manganese in permanganate is reduced from an oxidation state of +7 to +2, indicating a gain of electrons.
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Related Practice
Textbook Question
Consider the following half-reactions and E° values: (c) Write the cell reaction for part (b), and calculate the values of E°, ∆G° (in kilojoules), and K for this reaction at 25 °C
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Textbook Question
Chlorine can be prepared in the laboratory by the reaction of hydrochloric acid and potassium permanganate.(b) Calculate E° and ∆G° for the reaction
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Textbook Question
The sodium–sulfur battery has molybdenum electrodes with anode and cathode compartments separated by b-alumina, a ceramic through which sodium ions can pass. Because the battery operates at temperatures above 300 °C, all the reactants and products are present in a molten solution. The cell voltage is about 2.0 V. (b) How many kilograms of sodium are consumed when a 25 kW sodium–sulfur battery produces current for 32 min?
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Textbook Question
Given the following standard reduction potentials at 25 °C, (a) balance the equation for the reaction of H2MoO4 with elemental arsenic in acidic solution to give Mo3+ and H3AsO4 and (b) calculate E° for this reaction.
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