Textbook Question
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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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement143
- Ch.2 - Atoms, Molecules & Ions134
- Ch.3 - Mass Relationships in Chemical Reactions149
- Ch.4 - Reactions in Aqueous Solution157
- Ch.5 - Periodicity & Electronic Structure of Atoms92
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory73
- Ch.7 - Covalent Bonding and Electron-Dot Structures47
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure51
- Ch.9 - Thermochemistry: Chemical Energy104
- Ch.10 - Gases: Their Properties & Behavior138
- Ch.11 - Liquids & Phase Changes43
- Ch.12 - Solids and Solid-State Materials56
- Ch.13 - Solutions & Their Properties98
- Ch.14 - Chemical Kinetics79
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Aqueous Equilibria: Acids & Bases94
- Ch.17 - Applications of Aqueous Equilibria125
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium66
- Ch.19 - Electrochemistry130
- Ch.20 - Nuclear Chemistry73
- Ch.21 - Transition Elements and Coordination Chemistry122
- Ch.22 - The Main Group Elements155
- Ch.23 - Organic and Biological Chemistry43
Chapter 19, Problem 83c
What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (c) A silver wire is immersed in an aqueous solution of NiCl2.
Verified step by step guidance1
Identify the possible redox reaction: Silver (Ag) and Nickel (Ni) can potentially undergo a redox reaction. Silver can be reduced, and nickel can be oxidized.
Write the half-reactions: The reduction half-reaction for silver is Ag^+ + e^- → Ag, and the oxidation half-reaction for nickel is Ni → Ni^2+ + 2e^-.
Determine the standard electrode potentials: Look up the standard reduction potentials for Ag^+ to Ag and Ni^2+ to Ni. Ag^+ + e^- → Ag has a potential of +0.80 V, and Ni^2+ + 2e^- → Ni has a potential of -0.25 V.
Calculate the cell potential: Use the formula E°_cell = E°_cathode - E°_anode. Substitute the values to find the overall cell potential.
Analyze the feasibility: If the calculated E°_cell is positive, the reaction is spontaneous under standard conditions. If negative, no reaction occurs.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Standard-State Conditions
Standard-state conditions refer to a set of specific conditions used to measure the properties of substances. These typically include a temperature of 25°C (298 K), a pressure of 1 atm, and concentrations of 1 M for solutions. Understanding these conditions is crucial for predicting the behavior of chemical reactions and the feasibility of reactions under specified circumstances.
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Standard Reduction Potentials
Electrochemical Reactions
Electrochemical reactions involve the transfer of electrons between species, often occurring in redox (reduction-oxidation) processes. In the context of the silver wire and NiCl2 solution, it is important to consider the standard reduction potentials of silver and nickel ions to determine if a spontaneous reaction can occur. The relative positions of these potentials dictate whether one metal can displace another from its ionic form.
Displacement Reactions
Displacement reactions occur when a more reactive element displaces a less reactive element from its compound. In this scenario, if silver (Ag) is more reactive than nickel (Ni) in the context of their respective ions, a reaction will take place where silver ions are produced, and nickel is deposited. Understanding the reactivity series of metals is essential for predicting the outcome of such reactions.
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Calculate E° for each of the following reactions, and tell which are spontaneous under standard-state conditions.(a)
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