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
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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 43
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?
Guida verificata passo dopo passo1
Identify the balanced chemical equation: 2 \(\text{ZnS}\)(s) + 3 \(\text{O}\)_2(g) \(\rightarrow\) 2 \(\text{ZnO}\)(s) + 2 \(\text{SO}\)_2(g).
Determine the mole ratio from the balanced equation: 2 moles of ZnS react with 3 moles of O_2.
Calculate the moles of O_2 needed to completely react with 4.2 moles of ZnS using the mole ratio: \(\frac{3 \text{ moles O}\)_2}{2 \(\text{ moles ZnS}\)}.
Calculate the moles of ZnS needed to completely react with 6.8 moles of O_2 using the mole ratio: \(\frac{2 \text{ moles ZnS}\)}{3 \(\text{ moles O}\)_2}.
Compare the calculated moles of O_2 and ZnS needed to determine the limiting reactant and calculate the remaining moles of the excess reactant.
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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 find out how much of each reactant is consumed and how much remains after the reaction.
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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 calculating the amounts of excess reactants left over after the reaction. In this scenario, we need to determine which reactant, ZnS or O2, limits the reaction to find the excess.
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Percorso guidato
01:30Limiting Reagent Concept
Excess Reactant
An excess reactant is a reactant that remains after the reaction has gone to completion because it was not completely consumed. Understanding the concept of excess reactants is important for calculating how much of a particular reactant is left over after the reaction. In this problem, we will calculate the moles of the excess reactant remaining after the reaction between ZnS and O2.
Video consigliato:
Percorso guidato
01:30Limiting Reagent Concept
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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
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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?
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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: 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?
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