Domanda del libro di testo
Calculate the theoretical yield of the product (in moles) for each initial amount of reactants.
Ti(s) + 2 Cl2(g) → TiCl4(s)
a. 4 mol Ti, 4 mol Cl2
b. 7 mol Ti, 17 mol Cl2
c. 12.4 mol Ti, 18.8 mol Cl2
1693
views
Ch.4 - Chemical Quantities & Aqueous Reactions
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
Non è quello che usi tu?Cambia libro di testoScegli un libro di testo diverso
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 42
Calculate the theoretical yield of product (in moles) for each initial amount of reactants.
3 Mn(s) + 2 O2(g) → Mn3O4(s)
a. 3 mol Mn, 2 mol O2
b. 4 mol Mn, 7 mol O2
c. 27.5 mol Mn, 43.8 mol O2
Guida verificata passo dopo passo1
Identify the balanced chemical equation: 3 \(\text{ Mn}\)(s) + 2 \(\text{ O}\)_2(g) \(\rightarrow\) \(\text{ Mn}\)_3\(\text{O}\)_4(s)
Determine the molar ratio between reactants and product from the balanced equation: 3 \(\text{ mol Mn}\) : 2 \(\text{ mol O}\)_2 : 1 \(\text{ mol Mn}\)_3\(\text{O}\)_4
Calculate the theoretical yield of Mn_3O_4 based on the amount of Mn: \(\frac{4 \text{ mol Mn}\)}{3 \(\text{ mol Mn}\)} \(\times\) 1 \(\text{ mol Mn}\)_3\(\text{O}\)_4
Calculate the theoretical yield of Mn_3O_4 based on the amount of O_2: \(\frac{7 \text{ mol O}\)_2}{2 \(\text{ mol O}\)_2} \(\times\) 1 \(\text{ mol Mn}\)_3\(\text{O}\)_4
Identify the limiting reactant by comparing the theoretical yields from Mn and O_2, and use the smaller yield as the theoretical yield of Mn_3O_4.
Risposta video verificata per un problema simile:
Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Concetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
Stoichiometry
Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. It allows chemists to predict the amounts of substances consumed and produced in a given reaction based on balanced chemical equations. Understanding stoichiometry is essential for calculating theoretical yields, as it provides the mole ratios needed to determine how much product can be formed from specific amounts of reactants.
Video consigliato:
Percorso guidato
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 yield calculations, as it dictates the extent of the reaction. In the given question, one must compare the mole ratios of the reactants to find which one limits the formation of Mn3O4.
Video consigliato:
Percorso guidato
01:30Limiting Reagent Concept
Theoretical Yield
Theoretical yield is the maximum amount of product that can be generated from a given amount of reactants, assuming complete conversion and no losses. It is calculated using stoichiometric relationships derived from the balanced chemical equation. The theoretical yield is important for evaluating the efficiency of a reaction and is often compared to the actual yield obtained in practice to determine the reaction's success.
Video consigliato:
Percorso guidato
03:09Percent Yield in Reactions
Pratica correlata
Domanda del libro di testo
Zinc sulfide reacts with oxygen according to the reaction: 2 ZnS(s) + 3 O2(g) → 2 ZnO(s) + 2 SO2( g) A reaction mixture initially contains 4.2 mol ZnS and 6.8 mol O2. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains?
7103
views
1
comments
Domanda del libro di testo
Iron(II) sulfide reacts with hydrochloric acid according to the reaction: FeS(s) + 2 HCl(aq) → FeCl2(s) + H2S(g) A reaction mixture initially contains 0.223 mol FeS and 0.652 mol HCl. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains?
8939
views
1
rank
Domanda del libro di testo
Iron(II) sulfide reacts with hydrochloric acid according to the reaction: FeS(s) + 2 HCl(aq) → FeCl2(s) + H2S(g) A reaction mixture initially contains 0.223 mol FeS and 0.652 mol HCl. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains?
Domanda del libro di testo
Consider the reaction: 4 HCl(g) + O2(g) → 2 H2O(g) + 2 Cl2(g) Each molecular diagram represents an initial mixture of reactants. How many molecules of Cl2 form from the reaction mixture that produces the greatest amount of products?
2250
views
3
rank
Domanda del libro di testo
Consider the reaction: 2 CH3OH(g) + 3 O2(g) → 2 CO2(g) + 4 H2O(g) Each of the molecular diagrams represents an initial mixture of the reactants. How many CO2 molecules form from the reaction mixture that produces the greatest amount of products?
2725
views
1
comments