교과서 질문
What products are obtained in the electrolysis of a molten mixture of KI and KBr?
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Ch.20 - Electrochemistry
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
20장, 문제 100a
Write equations for the half-reactions that occur at the anode and cathode for the electrolysis of each aqueous solution. a. Ni(NO3)2(aq)
검증된 단계별 안내1
Step 1: Identify the ions present in the solution. In this case, the solution of Ni(NO3)2(aq) will dissociate into Ni2+ ions and NO3- ions.
Step 2: Determine the possible reactions at the anode and cathode. The anode is where oxidation occurs, and the cathode is where reduction occurs. In an aqueous solution, water can also be oxidized or reduced, producing O2 and H2 respectively.
Step 3: Write the half-reactions. For the anode (oxidation), the possible reactions are the oxidation of Ni2+ to Ni or the oxidation of water to O2. For the cathode (reduction), the possible reactions are the reduction of Ni2+ to Ni or the reduction of water to H2.
Step 4: Determine the most likely reactions based on the standard reduction potentials. The reaction with the higher reduction potential is more likely to occur at the cathode, and the reaction with the lower reduction potential is more likely to occur at the anode.
Step 5: Write the final half-reactions. The final half-reactions will depend on the standard reduction potentials of the possible reactions. Remember to balance the half-reactions by adding electrons to the appropriate side.
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이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.
영상 길이:
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주요 개념
질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.
Electrolysis
Electrolysis is a chemical process that uses electrical energy to drive a non-spontaneous reaction. In this process, an electric current is passed through an electrolyte, causing the decomposition of the compound into its constituent elements or ions. The reactions occur at two electrodes: the anode (oxidation) and the cathode (reduction), where different half-reactions take place.
추천 영상:
가이드 코스
01:21
The Electrolytic Cell
Half-Reactions
Half-reactions are the individual oxidation or reduction reactions that occur at the electrodes during electrolysis. Each half-reaction shows the transfer of electrons and the change in oxidation states of the species involved. For example, at the anode, a species may lose electrons (oxidation), while at the cathode, another species gains electrons (reduction).
추천 영상:
가이드 코스
01:49First-Order Half-Life
Electrolyte Solutions
Electrolyte solutions contain ions that can conduct electricity, allowing electrolysis to occur. In the case of Ni(NO3)2(aq), the solution dissociates into nickel ions (Ni²⁺) and nitrate ions (NO3⁻). The specific ions present in the solution will determine the products formed at the electrodes during electrolysis, influencing the half-reactions that need to be written.
추천 영상:
가이드 코스
02:50Electrolytes and Strong Acids