Textbook Question
Describe the reactions that occur when an Si1OH24 sol becomes a gel. What is the formula of the ceramic obtained when the gel is dried and sintered?
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Ch.12 - Solids and Solid-State Materials
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 12, Problem 134
The mineral magnetite is an iron oxide ore that has a density of 5.20 g/cm³. At high temperature, magnetite reacts with carbon monoxide to yield iron metal and carbon dioxide. When 2.660 g of magnetite is allowed to react with sufficient carbon monoxide, the CO₂ product is found to have a volume of 1.136 L at 298 K and 751 mm Hg pressure. (a) What mass of iron in grams is formed in the reaction? (b) What is the formula of magnetite?
Verified step by step guidance1
Step 1: Write the balanced chemical equation for the reaction of magnetite (Fe₃O₄) with carbon monoxide (CO) to produce iron (Fe) and carbon dioxide (CO₂).
Step 2: Use the ideal gas law, PV = nRT, to calculate the number of moles of CO₂ produced. Convert the pressure from mm Hg to atm and use R = 0.0821 L·atm/mol·K.
Step 3: Use stoichiometry to determine the moles of iron produced. From the balanced equation, find the mole ratio between CO₂ and Fe.
Step 4: Calculate the mass of iron produced using the moles of iron and the molar mass of iron (55.85 g/mol).
Step 5: Determine the formula of magnetite by recognizing it as Fe₃O₄, a common iron oxide mineral.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Stoichiometry
Stoichiometry is the calculation of reactants and products in chemical reactions based on the conservation of mass. It involves using balanced chemical equations to determine the relationships between the amounts of substances consumed and produced. In this question, stoichiometry will help calculate the mass of iron produced from the given mass of magnetite and the volume of carbon dioxide generated.
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Stoichiometry Concept
Ideal Gas Law
The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. This law is essential for converting the volume of carbon dioxide produced into moles, which can then be used in stoichiometric calculations. Understanding this concept is crucial for determining how much iron is formed from the reaction involving magnetite and carbon monoxide.
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Chemical Formula of Magnetite
The chemical formula of magnetite is Fe₃O₄, indicating that it is composed of three iron (Fe) atoms and four oxygen (O) atoms. Recognizing the formula is important for understanding the composition of the mineral and for performing stoichiometric calculations in the reaction with carbon monoxide. This knowledge is fundamental to answering part (b) of the question regarding the formula of magnetite.
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Related Practice
Textbook Question
Explain why silicon carbide–reinforced alumina is strongerand tougher than pure alumina.
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Textbook Question
A cube-shaped crystal of an alkali metal, 1.62 mm on an edge, was vaporized in a 500.0 mL evacuated flask. The resulting vapor pressure was 12.5 mm Hg at 802 °C. The structure of the solid metal is known to be body-centered cubic. (c) What are the densities of the solid and the vapor in g>cm3?
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Textbook Question
A group 3A metal has a density of 2.70 g/cm3 and a cubic unit cell with an edge length of 404 pm. Reaction of A 1.07 cm3 chunk of the metal with an excess of hydrochloric acid gives a colorless gas that occupies 4.00 L at 23.0 °C and a pressure of 740 mm Hg. (a) Identify the metal.
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Textbook Question
Assume that 1.588 g of an alkali metal undergoes complete reaction with the amount of gaseous halogen contained in a 0.500 L flask at 298 K and 755 mm Hg pressure. In the reaction, 22.83 kJ is released 1ΔH = -22.83 kJ2. The product, a binary ionic compound, crystallizes in a unit cell with anions in a face-centered cubic arrangement and with cations centered along each edge between anions. In addition, there is a cation in the center of the cube. (c) Sketch a space-filling, head-on view of the unit cell, labeling the ions. Are the anions in contact with one another?
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Textbook Question
Explain why graphite/epoxy composites are good materials for making tennis rackets and golf clubs.
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