Balance the following equation. Then, given the moles of reactant or product below, determine the corresponding amount in moles of each of the other reactants and products. NH3 + O2 N2 + H2O a. 4 mol NH3 b. 4 mol N2 c. 4.5 mol O2
Read moreTable of Contents
1
Matter andChange
1.1
Chemistry Is a Physical Science
1.2
Matter and Its Properties
1.3
Elements
2
Measurementsand Calculations
2.1
Scientific Method
2.2
Units of Measurement
2.3
Using Scientific Measurements
3
Standards-Based Assessment
3.1
The Atom: FromPhilosophical Ideato Scientific Theory
3.2
The Structure ofthe Atom
3.3
Counting Atoms
4
Arrangement ofElectrons inAtoms
4.1
The Development ofa New Atomic Model
4.2
The Quantum Modelof the Atom
4.3
Electron Configurations
5
The Periodic Law
5.1
History of the Periodic Table
5.2
ElectronConfiguration andthe Periodic Table
5.3
ElectronConfiguration andPeriodic Properties
6
Chemical Bonding
6.1
Introduction toChemical Bonding
6.2
Covalent Bondingand MolecularCompounds
6.3
Ionic Bonding andIonic Compounds
6.4
Metallic Bonding
6.5
Molecular Geometry
7
ChemicalFormulas andChemicalCompounds
7.1
Chemical Names and Formulas
7.2
Oxidation Numbers
7.3
Using Chemical Formulas
7.4
Determining Chemical Formulas
8
ChemicalEquationsand Reactions
8.1
Describing ChemicalReactions
8.2
Types of ChemicalReactions
8.3
Activity Series ofthe Elements
9
Stoichiometry
9.1
Introduction to Stoichiometry
9.2
Ideal StoichiometricCalculations
9.3
Limiting Reactantsand Percentage Yield
10
States of Matter
10.1
The Kinetic-Molecular Theoryof Matter
10.2
Liquids
10.3
Solids
10.4
Changes of State
10.5
Water
11
Gases
11.1
Gases and Pressure
11.2
The Gas Laws
11.3
Gas Volumes andthe Ideal Gas Law
11.4
Diffusion andEffusion
12
Solutions
12.1
Types of Mixtures
12.2
The SolutionProcess
12.3
Concentration ofSolutions
13
Ions in AqueousSolutions andColligativeProperties
13.1
Compounds in Aqueous Solutions
13.2
ColligativeProperties ofSolutions
14
Acids and Bases
14.1
Properties of Acids and Bases
14.2
Acid-Base Theories
14.3
Acid-Base Reactions
15
Acid-Base Titrationand pH
15.1
Aqueous Solutionsand the Conceptof pH
15.2
Determining pHand Titrations
16
Reaction Energy
16.1
Thermochemistry
16.2
Driving Force of Reactions
17
Kinetic Reactions
17.1
The Reaction Process
17.2
Reaction Rate
18
Chemical Equilibrium
18.1
The Nature of Chemical Equilibrium
18.2
Shifting Equilibrium
18.3
Equilibria of Acids, Bases, and Salts
18.4
Solubility Equilibrium
19
Oxidation-Reduction Reactions
19.1
Oxidation and Reduction
19.2
Balancing Redox Equations
19.3
Oxidizing and Reducing Agents
20
Electrochemistry
20.1
Introduction to Electrochemistry
20.2
Voltaic Cells
20.3
Electrolytic Cells
21
Nuclear Chemistry
21.1
The Nucleus
21.2
Radioactive Decay
21.3
Nuclear Radiation
21.4
Nuclear Fission and Nuclear Fusion
22
Organic Chemistry
22.1
Organic Compounds
22.2
Hydrocarbons
22.3
Functional Groups
22.4
Organic Reactions
23
Biological Chemistry
23.1
Carbohydrates and Lipids
23.2
Amino Acids and Proteins
23.3
Metabolism
23.4
Nucleic Acids
Textbook Solutions for Modern Chemistry: Student Edition 2012
Chapter 9.2 Problem 9.1.7
Question
Acetylene gas, C2H2, is produced as a result of the following reaction: CaC2(s) + 2H2O(l) C2H2(g) + Ca(OH)2(aq) a. If 32.0 g CaC2 are consumed in this reaction, how many moles of H2O are needed? b. How many moles of each product would form?
Solution
The first step in solving 9.2 problem number 3 trying to solve the problem we have to refer to the textbook question: Acetylene gas, C2H2, is produced as a result of the following reaction: CaC2(s) + 2H2O(l) C2H2(g) + Ca(OH)2(aq) a. If 32.0 g CaC2 are consumed in this reaction, how many moles of H2O are needed? b. How many moles of each product would form?
From the textbook chapter Ideal StoichiometricCalculations you will find a few key concepts needed to solve this.
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Title
Modern Chemistry: Student Edition 2012 1
Author
Jerry L. Sarquis, Mickey Sarquis
ISBN
9780547586632
Acetylene gas, C2H2, is produced as a result of the
Chapter 9.2 textbook questions
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Chapter 9: Problem 9 Modern Chemistry: Student Edition 2012 1
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Chapter 9: Problem 9 Modern Chemistry: Student Edition 2012 1
One reaction that produces hydrogen gas can be represented by the following unbalanced chemical equation: Mg(s) + HCl(aq) MgCl2(aq) + H2(g) a. What mass of HCl is consumed by the reaction of 2.50 moles of magnesium? b. What mass of each product is produced in part (a)?
Read more -
Chapter 9: Problem 9 Modern Chemistry: Student Edition 2012 1
Acetylene gas, C2H2, is produced as a result of the following reaction: CaC2(s) + 2H2O(l) C2H2(g) + Ca(OH)2(aq) a. If 32.0 g CaC2 are consumed in this reaction, how many moles of H2O are needed? b. How many moles of each product would form?
Read more -
Chapter 9: Problem 9 Modern Chemistry: Student Edition 2012 1
When sodium chloride reacts with silver nitrate, silver chloride precipitates. What mass of AgCl is produced from 75.0 g AgNO3?
Read more -
Chapter 9: Problem 9 Modern Chemistry: Student Edition 2012 1
RELATING IDEAS Carbon and oxygen react to form carbon monoxide: 2C + O2 2CO. What masses of carbon and oxygen are needed to make 56.0 g CO? Which law does this illustrate?
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