Domanda del libro di testo
What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (d) A nickel wire is dipped into an aqueous solution of HClO.
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Ch.19 - Electrochemistry
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- 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
Capitolo 19, Problema 83a
What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (a) A strip of zinc is dipped into an aqueous solution of Pb(NO3)2.
Guida verificata passo dopo passo1
Identify the reactants involved in the experiment: zinc metal (Zn) and lead(II) nitrate (Pb(NO3)2).
Write down the possible half-reactions for each reactant. For zinc, it can oxidize, losing electrons: Zn(s) → Zn^2+(aq) + 2e^-. For lead(II) nitrate, the lead(II) ions can reduce, gaining electrons: Pb^2+(aq) + 2e^- → Pb(s).
Consult the standard reduction potential table to find the values for each half-reaction. The standard reduction potential for the zinc reaction (as an oxidation) is -0.76 V and for the lead reaction (as a reduction) is -0.13 V.
Compare the reduction potentials to determine the feasibility of the reaction. The substance with the higher (less negative) reduction potential will undergo reduction, while the other will undergo oxidation.
Conclude that since the reduction potential of lead(II) is higher than that of zinc, lead(II) ions will be reduced to lead metal, and zinc metal will be oxidized to zinc ions. Thus, a redox reaction will occur where zinc displaces lead from its nitrate solution.
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Redox Reactions
Redox reactions involve the transfer of electrons between substances, leading to changes in oxidation states. In the context of the question, zinc (Zn) can act as a reducing agent, losing electrons, while lead ions (Pb^2+) can gain electrons, thus being reduced. Understanding the principles of oxidation and reduction is essential for predicting the outcome of the reaction.
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Percorso guidato
03:12
Identifying Redox Reactions
Standard-State Conditions
Standard-state conditions refer to a set of specific conditions (1 atm pressure, 25°C temperature, and 1 M concentration for solutions) under which the properties of substances are measured. These conditions provide a consistent framework for comparing thermodynamic data and predicting the feasibility of reactions, such as the one between zinc and lead nitrate.
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Percorso guidato
01:10Standard Reduction Potentials
Activity Series of Metals
The activity series is a list of metals ranked by their ability to displace other metals from solutions of their ions. Zinc is more reactive than lead, meaning it can displace lead ions from the solution. This concept is crucial for determining whether a reaction will occur when zinc is placed in a solution of Pb(NO3)2.
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02:02Activity Series Chart
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