Domanda del libro di testo
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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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 151
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?
Guida verificata passo dopo passo1
Step 1: Calculate the total energy produced by the battery. Use the formula: Energy (in kWh) = Power (in kW) × Time (in hours). Convert 32 minutes into hours.
Step 2: Convert the energy from kWh to joules. Use the conversion factor: 1 kWh = 3.6 × 10^6 J.
Step 3: Calculate the total charge (in coulombs) using the formula: Charge (Q) = Energy (in joules) / Voltage (in volts). Here, the voltage is given as 2.0 V.
Step 4: Use Faraday's laws of electrolysis to find the moles of sodium consumed. The formula is: Moles of Na = Charge (Q) / (n × F), where n is the number of electrons transferred per mole of Na (n = 1 for Na), and F is Faraday's constant (approximately 96485 C/mol).
Step 5: Convert the moles of sodium to mass in kilograms. Use the molar mass of sodium (approximately 22.99 g/mol) and convert grams to kilograms.
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Electrochemical Cells
Electrochemical cells, such as batteries, convert chemical energy into electrical energy through redox reactions. In a sodium-sulfur battery, sodium ions move through a ceramic electrolyte, allowing for the flow of electric current. Understanding the operation of these cells is crucial for calculating the amount of reactants consumed during the battery's operation.
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Percorso guidato
02:46
Electrochemical Cells
Current and Charge
Current is the flow of electric charge, measured in amperes (A), and is related to the amount of charge (in coulombs) that passes through a circuit over time. The relationship between current, charge, and time is given by the equation Q = I × t, where Q is charge, I is current, and t is time. This concept is essential for determining how much sodium is consumed based on the current produced by the battery.
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Percorso guidato
01:53Formal Charge
Molar Mass and Stoichiometry
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole. Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced equations. In this context, knowing the molar mass of sodium allows for the conversion of the total charge produced by the battery into the mass of sodium consumed, facilitating the final calculation.
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Percorso guidato
02:11Molar Mass Concept
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Domanda del libro di testo
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Domanda del libro di testo
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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