Domanda del libro di testo
Predict the anode, cathode, and overall cell reactions when an aqueous solution of each of the following salts is electrolyzed in a cell having inert electrodes. (c) LiOH
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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 140
How many hours are required to produce 1.00 * 103 kg of sodium by the electrolysis of molten NaCl with a constant current of 3.00 * 104 A? How many liters of Cl2 at STP will be obtained as a by-product?
Guida verificata passo dopo passo1
Identify the chemical reaction involved in the electrolysis of molten NaCl: \(2\text{NaCl} \rightarrow 2\text{Na} + \text{Cl}_2\).
Calculate the moles of sodium (Na) to be produced using its molar mass: \(\text{moles of Na} = \frac{\text{mass of Na}}{\text{molar mass of Na}}\).
Determine the moles of electrons required using the stoichiometry of the reaction: 2 moles of electrons are needed to produce 2 moles of Na.
Use Faraday's law of electrolysis to find the total charge required: \(Q = n \times F\), where \(n\) is the moles of electrons and \(F\) is Faraday's constant (96485 C/mol).
Calculate the time in seconds using the formula \(t = \frac{Q}{I}\), where \(I\) is the current, and then convert the time from seconds to hours.
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Electrolysis
Electrolysis is a chemical process that uses electrical energy to drive a non-spontaneous reaction. In the case of molten NaCl, electrolysis separates sodium ions (Na+) and chloride ions (Cl-) at the anode and cathode, respectively. This process is essential for producing sodium metal and chlorine gas from sodium chloride.
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Percorso guidato
01:21
The Electrolytic Cell
Faraday's Laws of Electrolysis
Faraday's Laws of Electrolysis quantify the relationship between the amount of substance produced at an electrode and the electric charge passed through the electrolyte. The first law states that the mass of a substance produced is directly proportional to the electric charge. This principle is crucial for calculating the time required for electrolysis based on current and the amount of sodium desired.
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Percorso guidato
01:40Faraday's Constant in Electrochemistry
Stoichiometry of Gases
Stoichiometry of gases involves the relationships between the volumes of gases and the amounts of substances in a chemical reaction, particularly under standard temperature and pressure (STP). At STP, one mole of any gas occupies 22.4 liters. This concept is vital for determining the volume of chlorine gas produced as a by-product during the electrolysis of NaCl.
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Percorso guidato
01:16Stoichiometry Concept
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