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A mixture of FeO and Fe2O3 with a mass of 10.0 g is con-verted to 7.43 g of pure Fe metal. What are the amounts in grams of FeO and Fe2O3 in the original sample?
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Ch.3 - Mass Relationships in Chemical Reactions
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
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McMurry 8th EditionCh.3 - Mass Relationships in Chemical ReactionsProblema 115
McMurry 8th EditionCh.3 - Mass Relationships in Chemical ReactionsProblema 115Capitolo 3, Problema 115
A compound of formula XCl3 reacts with aqueous AgNO3 to yield solid AgCl according to the following equation: When a solution containing 0.634 g of XCl3 was allowed to react with an excess of aqueous AgNO3, 1.68 g of solid AgCl was formed. What is the identity of the atom X?
Guida verificata passo dopo passo1
Write the balanced chemical equation for the reaction: \[ \text{XCl}_3 + 3\text{AgNO}_3 \rightarrow 3\text{AgCl} + \text{X(NO}_3\text{)}_3 \]
Calculate the moles of AgCl formed using its molar mass: \[ \text{moles of AgCl} = \frac{1.68 \text{ g}}{\text{molar mass of AgCl}} \]
Use the stoichiometry of the balanced equation to find the moles of XCl3 that reacted. Since 3 moles of AgCl are produced per mole of XCl3, divide the moles of AgCl by 3.
Calculate the molar mass of XCl3 using the mass of XCl3 and the moles calculated: \[ \text{molar mass of XCl}_3 = \frac{0.634 \text{ g}}{\text{moles of XCl}_3} \]
Subtract the molar mass of 3 Cl atoms from the molar mass of XCl3 to find the atomic mass of X, and identify the element X based on its atomic mass.
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Stoichiometry
Stoichiometry is the calculation of reactants and products in chemical reactions. It involves using balanced chemical equations to determine the relationships between the amounts of substances consumed and produced. In this question, stoichiometry will help relate the mass of XCl3 to the mass of AgCl formed, allowing for the identification of the element X.
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Percorso guidato
01:16
Stoichiometry Concept
Molar Mass
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is crucial for converting between the mass of a substance and the number of moles, which is necessary for stoichiometric calculations. Knowing the molar mass of AgCl and the mass of AgCl produced will help determine the moles of XCl3 that reacted.
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Percorso guidato
02:11Molar Mass Concept
Chemical Identity and Valency
The chemical identity of an element refers to its unique properties and position in the periodic table, while valency indicates the combining capacity of an element. In this case, understanding the valency of the element X in XCl3 is essential to deduce its identity based on the number of chloride ions it can bond with, which is critical for determining the element X when combined with AgNO3.
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Percorso guidato
02:12Transition Metals Valence Electrons
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A copper wire having a mass of 2.196 g was allowed to react with an excess of sulfur. The excess sulfur was then burned, yielding SO2 gas. The mass of the copper sulfide produced was 2.748 g. (a) What is the percent composition of copper sulfide?
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Domanda del libro di testo
A copper wire having a mass of 2.196 g was allowed to react with an excess of sulfur. The excess sulfur was then burned, yielding SO2 gas. The mass of the copper sulfide produced was 2.748 g. (b) What is its empirical formula?
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A pulverized rock sample believed to be pure calcium carbonate, CaCO3, is subjected to chemical analysis and found to contain 51.3% Ca, 7.7% C, and 41.0% O by mass. Why can't this rock sample be pure CaCO3?
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A certain alcoholic beverage contains only ethanol (C2H6O) and water. When a sample of this beverage undergoes com-bustion, the ethanol burns but the water simply evaporates and is collected along with the water produced by combus-tion. The combustion reaction is
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When eaten, dietary carbohydrates are digested to yield glu-cose (C6H12O6), which is then metabolized to yield carbon dioxide and water:
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