Domanda del libro di testo
For the reaction shown, calculate the theoretical yield of product (in grams) for each initial amount of reactants. 2 Al(s) + 3 Cl2(g) → 2 AlCl3(s) c. 0.235 g Al, 1.15 g Cl2
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Ch.4 - Chemical Quantities & Aqueous Reactions
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving136
- Ch.2 - Atoms & Elements112
- Ch.3 - Molecules, Compounds & Chemical Equations159
- Ch.4 - Chemical Quantities & Aqueous Reactions140
- Ch.5 - Gases118
- Ch.6 - Thermochemistry106
- Ch.7 - Quantum-Mechanical Model of the Atom62
- Ch.8 - Periodic Properties of the Elements103
- Ch.9 - Chemical Bonding I: The Lewis Model104
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory89
- Ch.11 - Liquids, Solids & Intermolecular Forces73
- Ch.12 - Solids and Modern Material59
- Ch.13 - Solutions110
- Ch.14 - Chemical Kinetics140
- Ch.15 - Chemical Equilibrium78
- Ch.16 - Acids and Bases155
- Ch.17 - Aqueous Ionic Equilibrium176
- Ch.18 - Free Energy and Thermodynamics108
- Ch.19 - Electrochemistry118
- Ch.20 - Radioactivity and Nuclear Chemistry82
- Ch.21 - Organic Chemistry150
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Capitolo 4, Problema 47
Iron(III) oxide reacts with carbon monoxide according to the equation: Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) A reaction mixture initially contains 22.55 g Fe2O3 and 14.78 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?
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Calculate the molar mass of Fe_2O_3 and CO using the periodic table.
Convert the given masses of Fe_2O_3 and CO to moles by dividing by their respective molar masses.
Determine the limiting reactant by comparing the mole ratio of Fe_2O_3 to CO from the balanced equation with the mole ratio from the initial amounts.
Use the stoichiometry of the reaction to calculate how much of the excess reactant is consumed by the limiting reactant.
Subtract the moles of the excess reactant consumed from the initial moles to find the remaining moles, then convert this back to grams using the molar mass.
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Stoichiometry
Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to determine the proportions of substances involved in a reaction, which is essential for identifying limiting and excess reactants. In this case, stoichiometry will help us calculate how much of each reactant is consumed and how much remains after the reaction.
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01:16
Stoichiometry Concept
Limiting Reactant
The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is crucial for calculating the amounts of products and any excess reactants left over. In this reaction, we will need to find out which reactant, Fe2O3 or CO, limits the formation of iron and carbon dioxide.
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Percorso guidato
01:30Limiting Reagent Concept
Excess Reactant
The excess reactant is the substance that remains after the reaction has gone to completion, as it is not completely consumed. Understanding the concept of excess reactants is important for calculating how much of a reactant is left over after the reaction. In this scenario, once we identify the limiting reactant, we can determine the mass of the excess reactant that remains unreacted.
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Percorso guidato
01:30Limiting Reagent Concept
Pratica correlata
Domanda del libro di testo
Elemental phosphorus reacts with chlorine gas according to the equation: P4(s) + 6 Cl2( g) → 4 PCl3(l) A reaction mixture initially contains 45.69 g P4 and 131.3 g Cl2. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?
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Domanda del libro di testo
For the reaction shown, calculate the theoretical yield of the product (in grams) for each initial amount of reactants. Ti(s) + 2 F2( g) → TiF4(s) c. 0.233 g Ti, 0.288 g F2
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Domanda del libro di testo
Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is: 2 Mg(s) + O2(g) → 2 MgO(s) When 10.1 g of Mg reacts with 10.5 g O2, 11.9 g MgO is collected. Determine the limiting reactant, theoretical yield, and percent yield for the reaction.
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