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Phase Diagram

Q. A phase diagram is a pressure-temperature graph that shows the rangers of temperature and pressure over which each phase is stable. The phase diagram is divided into three regions, each region representing one stable phase: solid, liquid, or gas. There are three boundary lines that separate the phases from one another. These boundary lines represent the equilibrium between two phases. the point at which the three boundary lines intersect is called the triple point. All three phases can exist in equilibrium with each other at this point. Select the image to explore the interactive activity that shows the phase diagram for CO2. Using the interactive diagram, you can observe what the phase of CO2 is at a particular temperature and pressure by moving the cursor to that point on the phase diagram. The animation also shows the type of movement experienced by CO2 molecules in a particular phase. You are given six samples of carbon dioxide (CO2) that are stored at different temperatures and at different pressures. Using the interactive activity showing the phase diagram of CO2, determine the phases of each of the samples and classify them according to which phase they are in. Keep in mind that the temperature and pressure are not to scale. Drag the appropriate items to their respective bins.

Solved • Jan 20, 2020

Phase Diagram

Q. The triple point of water is 0.0098 °C at 0.00603 atm (4.58 torr). At the triple point, ice, water, and water vapor exist in equilibrium with each other. Complete the following sentences to identify the process that ice, water, or water vapor may undergo if either the temperature or the pressure is increased. Match the words in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before submitting your answer.

Solved • Jan 20, 2020

Density

Q. Student Z completes his/her calibration step for part 3 and finds an average massA to be 95.237 g ± 0.005 g. However, in his/her calculations, s/he mistakenly uses 85.237 g ± 0.005 g for massA. S/he uses the correct values for massB and mass cyl. Will the calculated density be too high, too low, or unchanged?

Solved • Jan 20, 2020

Phase Diagram

Q. A phase diagram is a temperature-pressure plot that summarizes the conditions under which a substance exists as a solid, liquid, or gas. The curves that separate the phases are known as phase boundaries. Each phase boundary represents the equilibrium between the phases on either side of the curve. Identify the components of the phase diagram of water. Drag the appropriate labels to their respective targets.

Solved • Jan 20, 2020

Entropy

Q. The enthalpy of vaporization of water at 100.0°C is 40.68 kJ/mol. What is the entropy change in the surroundings when one mole of water vapor condenses at 100.0°C in a large room maintained at a temperature of 25.00°C? A.−136.4 J/ K . D.+109.0J / K B.−109.0J/ K . E.+136.4 J / K . C.−40.68 J / K

Solved • Jan 20, 2020

Phase Diagram

Q. Point A to G are located on the phase diagram of water. Which of the following statements are correct regarding navigation from one point to another across the phase diagram? Check all that apply.

Solved • Jan 20, 2020

Phase Diagram

Q. A phase diagram is a temperature-pressure plot that summarizes the conditions under which a substance exists as a solid, liquid, or gas. The curves that separate the phases are known as phase boundaries. Each phase boundary represents the equilibrium between the phases on either side of the curve. Identify the components of the phase diagram of water. Drag the appropriate labels to their respective targets.

Solved • Jan 20, 2020

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Ch.1 - Intro to General Chemistry
The Scientific Method Mixtures Scientific Notation Accuracy & Precision Standard Deviation, Mean, Median & Mode Metric Prefixes Significant Figures Energy, Heat and Temperature Physical & Chemical Changes Physical & Chemical Properties Types of Energy Dimensional Analysis Density
Ch.2 - Atoms & Elements
Periodic Table Periodic Table Charges Mole Concept Calculating Molar Mass Isotopes Subatomic Particles Atomic Theory Oil Drop Experiment
Ch.3 - Chemical Reactions
Ionic and Covalent Bonds Molecular Models Polyatomic Ions Naming Covalent Compounds Naming Ionic Compounds Naming Acids Empirical Formula Molecular Formula Combustion Analysis Mass Percent Formula Balancing Chemical Equations Functional Groups in Chemistry Stoichiometry Theoretical Yield Limiting Reagent Limiting Reactant Percent Yield
BONUS: Lab Techniques and Procedures
Distillation & Floatation Test for Ions and Gases
BONUS: Mathematical Operations and Functions
Multiplication and Division Operations
Ch.4 - Chemical Quantities & Aqueous Reactions
Molarity Normality & Equivalent Weight Solution Stoichiometry Dilution Solubility Rules Net Ionic Equations Net Ionic Equation Electrolytes Redox Reaction Balancing Redox Reactions Redox Reactions Oxidation Reduction (Redox) Reactions Calculate Oxidation Number Oxidation Number Types of Chemical Reactions Activity Series
Ch.5 - Gases
Pressure Units Manometer Partial Pressure The Ideal Gas Law Chemistry Gas Laws Ideal Gas Law Boyle's Law Ideal Gas Law Density Ideal Gas Law Molar Mass Standard Temperature and Pressure Gas Stoichiometry Collecting Gas Over Water Effusion Root Mean Square Speed Kinetic Molecular Theory Van der Waals Equation Kinetic Energy of Gases Velocity Distribution Charles Law Combined Gas Law
Ch.6 - Thermochemistry
Units of Energy Internal Energy Endothermic & Exothermic Reactions Calorimetry Thermochemical Equation Hess's Law Enthalpy of Formation Enthalpy
Ch.7 - Quantum Mechanics
Electromagnetic Spectrum Wavelength and Frequency Diffraction vs Refraction The Particle Nature of Light Photoelectric Effect De Broglie Wavelength Heisenberg Uncertainty Principle Bohr Model Bohr and Balmer Equations Wave Function Introduction to Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Electron Configuration Orbital Diagrams Paramagnetic and Diamagnetic Coulomb's Law Effective Nuclear Charge Quantum Numbers The Spin Quantum Number Orbital Shapes Periodic Trends Atomic Radius Periodic Trends: Atomic Radius Periodic Trends: Ionic Radius Periodic Trends: Ionization Energy Ionization Energy Periodic Trends: Electron Affinity Periodic Trends: Metallic Character Periodic Trend: Noble Gases
Ch.9 - Bonding & Molecular Structure
Chemical Bonds Lattice Energy Lattice Energy Application Born Haber Cycle Dipole Moment Lewis Dot Structure Octet Rule Formal Charge Resonance Structures Bond Energy
Ch.10 - Molecular Shapes & Valence Bond Theory
Molecular vs Electron Geometry Molecular Geometry VSEPR Theory Bond Angles Electronegativity Hybridization Benzene Orbital Overlap Molecular Orbital Theory Bond Order Delocalized Electrons Homonuclear Diatomic Molecules Heteronuclear Diatomic Molecules
Ch.11 - Liquids, Solids & Intermolecular Forces
Molecular Polarity Intermolecular Forces Intermolecular Forces and Physical Properties Phase Diagram Heating and Cooling Curves Unit Cell Atomic, Ionic, and Molecular Solids Clausius-Clapeyron Equation
Ch.12 - Solutions
Solutions, Molarity and Intermolecular Forces Making Solutions Henry's Law Calculate Molarity Mass Percent Molality Mole Fraction ppm Boiling Point Elevation Freezing Point Depression The Colligative Properties
Ch.13 - Chemical Kinetics
Rate of Reaction Average Rate of Reaction Instantaneous Rate of Change Arrhenius Equation Energy Diagram Catalyst Reaction Mechanism Rate Law Integrated Rate Law Identifying Reaction Order Collision Theory
Ch.14 - Chemical Equilibrium
Chemical Equilibrium Equilibrium Expressions ICE Chart Le Chatelier's Principle The Reaction Quotient
Ch.15 - Acid and Base Equilibrium
Identifying Acids and Bases Strong Acids and Strong Bases Arrhenius Acid and Base Bronsted Lowry Acid and Base Conjugate Acids and Bases Amphoteric Lewis Acid and Base pH and pOH Strong Acid-Base Calculations Weak Acids Weak Bases Ka and Kb Ionic Salts Diprotic Acid Polyprotic Acid
Ch.16 - Aqueous Equilibrium
Buffer Henderson Hasselbalch Equation Acid and Base Titration Curves Weak Acid Strong Base Titrations Weak Base Strong Acid Titrations Equivalence Point Strong Acid Strong Base Titrations Titrations of Diprotic and Polyprotic Acids Acid Base Indicators Ksp Selective Precipitation Formation Constant
Ch. 17 - Chemical Thermodynamics
Spontaneous Reaction First Law of Thermodynamics Second and Third Laws of Thermodynamics Entropy Boltzmann Equation Gibbs Free Energy
Ch.18 - Electrochemistry
Redox Reaction Balancing Redox Reaction The Nernst Equation Faraday's Constant Galvanic Cell Cell Notation Standard Hydrogen Electrode Cell Potential Nernst Equation Batteries and Electricity Electroplating Electrolysis of Water & Mixture of Ions
Ch.19 - Nuclear Chemistry
Radioactive Decay Alpha Decay Beta Decay Gamma Emission Electron Capture Positron Emission Band of Stability Magic Numbers First Order Half Life Nuclear Fission Mass Defect Nuclear Fusion Nuclear Transmutation
Ch.20 - Organic Chemistry
Introduction to Organic Chemistry Structural Formula Stereoisomers Chirality Optical Isomers The Alkyl Group Naming Alkanes Naming Alkenes Naming Alkynes Organic Chemistry Nomenclature Alkane Reactions Alkenes and Alkynes Functional Groups Alcohol Reactions Carboxylic Acid Derivative Reactions Polymer
Ch.22 - Chemistry of the Nonmetals
Alkali Metals
Ch.23 - Transition Metals and Coordination Compounds
Transition Metals Transition Metals Electron Configuration Oxidation States of Transition Metals Coordination Complexes Naming Coordination Compounds Coordination Isomers Crystal Field Theory Colors of Complex Ions