A Kinetics Problem (14.2.3) Flashcards by Anton Soloshenko | Brainscape

Q

• The equations ln[A]t = –kt + ln[A]0 and t1/2 = 0.693/k can be used to solve problems involving first-order reactions.

A

• The equations ln[A]t = –kt + ln[A]0 and t1/2 = 0.693/k can be used to solve problems involving first-order reactions.

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AP Chemistry (252 decks)

An Introduction to Chemistry (1.1.1)

The Scientific Method (1.1.2)

States of Matter (1.2.1)

A Word About Laboratory Safety (1.2.2)

CIA Demonstration: Differences in Density Due to Temperature (1.2.3)

Properties of Matter (1.2.4)

The Measurement of Matter (1.3.1)

Precision and Accuracy (1.3.2)

CIA Demonstration: Precision and Accuracy with Glassware (1.3.3)

Significant Figures (1.3.4)

Dimensional Analysis (1.3.5)

Scientific (Exponential) Notation (1.4.1)

Common Mathematical Functions (1.4.2)

Early Discoveries and the Atom (2.1.1)

Understanding Electrons (2.1.2)

Understanding the Nucleus (2.1.3)

Mass Spectrometry: Determining Atomic Masses (2.2.1)

Examining Atomic Structure (2.2.2)

CIA Demonstration: Flame Colors (2.2.3)

Creating the Periodic Table (2.3.1)

Describing Chemical Formulas (2.4.1)

Naming Chemical Compounds (2.4.2)

Organic Nomenclature (2.4.3)

An Introduction to Chemical Reactions and Equations (3.1.1)

CIA Demonstration: Magnesium and Dry Ice (3.1.2)

Balancing Chemical Equations (3.1.3)

The Mole and Avogadro's Number (3.2.1)

Introducing Conversions of Masses, Moles, and Number of Particles (3.2.2)

Finding Emperical and Molecular Formulas (3.3.1)

Stoichiometry and Chemical Equations (3.3.2)

Finding Limiting Reagents (3.3.3)

CIA Demonstration: Self-Inflating Hydrogen Balloons (3.3.4)

Theoretical Yield and Percent Yield (3.3.5)

A Problem Using the Combined Concepts of Stoichiometry (3.3.6)

Calculating Mass Percent (3.3.7)

Properties of Solutions (4.1.1)

CIA Demonstration: The Electric Pickle (4.1.2)

Concentrations of Solutions (4.1.3)

Factors Determining Solubility (4.1.4)

Precipitation Reactions (4.2.1)

Acid-Base Reactions (4.2.2)

Oxidation-Reduction Reactions (4.2.3)

Acid-Base Titrations (4.3.1)

Solving Titration Problems (4.3.2)

Gravimetric Analysis (4.3.3)

Properties of Gases (5.1.1)

Boyle's Law (5.1.2)

Charles's Law (5.1.3)

The Combined Gas Law (5.1.4)

Avogadro's Law (5.1.5)

CIA Demonstration: The Potato Cannon (5.1.6)

The Ideal Gas Law (5.2.1)

Partial Pressure and Dalton's Law (5.2.2)

Applications of the Gas Laws (5.2.3)

The Kinetic-Molecular Theory of Gases (5.2.4)

CIA Demonstration: The Ammonia Fountain (5.2.5)

Molecular Speeds (5.3.1)

Effusion and Diffusion (5.3.2)

Comparing Real and Ideal Gases (5.4.1)

The Nature of Energy (6.1.1)

Energy, Calories, and Nutrition (6.1.2)

The First Law of Thermodynamics (6.1.3)

CIA Demonstration: Cool Fire (6.1.6)

Heats of Reaction: Enthalpy (6.2.1)

CIA Demonstration: The Thermite Reaction (6.2.2)

Constant Pressure Calorimetry (6.3.1)

Bomb Calorimetry (Constant Volume) (6.3.2)

Hess's Law (6.4.1)

Enthalpies of Formation (6.4.2)

The Wave Nature of Light (7.1.1)

Absorption and Emission (7.1.2)

CIA Demonstration: Luminol (7.1.3)

The Ultraviolet Catastrophe (7.1.4)

The Photoelectric Effect (7.1.5)

The Bohr Model (7.1.6)

The Heisenberg Uncertainty Principle (7.1.7)

The Wave Nature of Matter (7.2.1)

Radial Solutions to the Schrodinger Equation (7.2.2)

Angular Solutions to the Schrodinger Equation (7.2.3)

Atomic Orbital Size (7.3.1)

Atomic Orbital Shapes and Quantum Numbers (7.3.2)

Atomic Orbital Energy (7.3.3)

Understanding Electron Spin (8.1.1)

Electron Shielding (8.1.2)

Electron Configurations Through Neon (8.1.3)

Electron Configurations Beyond Neon (8.1.4)

Periodic Relationships (8.1.5)

Periods and Atomic Size (8.2.1)

Ionization Energy (8.2.2)

Electron Affinity (8.2.3)

An Introduction to Electronegativity (8.2.4)

Hydrogen, Alkali Metals, and Alkaline Earth Metals (8.3.1)

Transition Metals and Nonmetals (8.3.2)

Valence Electrons and Chemical Bonding (9.1.1)

Ionic Bonds (9.1.2)

CIA Demonstration: Conductivity Apparatus-Ionic versus Covalent Bonds (9.1.3)

Lewis Dot Structures for Covalent Bonds (9.2.1)

Predicting Lewis Dot Structures (9.2.2)

Resonance Structures (9.3.1)

Formal Charge (9.3.2)

Electronegativity, Formal Charge, and Resonance (9.3.3)

Bond Properties (9.4.1)

Using Bond Dissociation Energies (9.4.2)

Valence-Shell Electron-Pair Repulsion Theory (10.1.1)

Molecular Shapes for Steric Numbers 2-4 (10.1.2)

Molecular Shapes for Steric Numbers 5 & 6 (10.1.3)

Predicting Molecular Characteristics Using VSEPR Theory (10.1.4)

Molecular Shapes: The AXE Method, Part 1 (10.1.5)

Molecular Shapes: The AXE Method, Part 2 (10.1.6)

Valence Bond Theory (10.2.1)

An Introduction to Hybrid Orbitals (10.2.2)

Pi Bonds (10.2.3)

Molecular Orbital Theory (10.2.4)

Applications of the Molecular Orbital Theory (10.2.5)

Beyond Homonuclear Diatomics (10.2.6)

CIA Demonstration: The Paramagnetism of Oxygen (10.2.7)

Oxidation Numbers (11.1.1)

Balancing Redox Reactions by the Oxidation Number Method (11.1.2)

Balancing Redox Reactions Using the Half-Reaction Method (11.1.3)

The Activity Series of the Elements (11.1.4)

CIA Demonstration: The Reaction Between Al and Br2 (11.1.5)

An Introduction to Intermolecular Forces and States of Matter (12.1.1)

Intermolecular Forces (12.1.2)

Properties of Liquids (12.2.1)

CIA Demonstration: Boiling Water at Reduced Pressure (12.2.2)

Vapor Pressure and Boiling Point (12.2.3)

Molecular Structure and Boiling Point (12.2.4)

Phase Diagrams (12.2.5)

CIA Demonstration: Boiling Water in a Paper Cup (12.2.6)

Types of Solids (12.3.1)

CIA Demonstration: The Conductivity of Molten Salts (12.3.2)

Crystal Structure (12.3.3)

Calculating Atomic Mass and Radius from a Unit Cell (12.3.4)

Crystal Packing (12.3.5)

Types of Solutions (13.1.1)

Molarity and the Mole Fraction (13.1.2)

Molality (13.1.3)

Energy and the Solution Process (13.1.4)

Temperature Change and Solubility (13.2.1)

Extractions (13.2.2)

Pressure Change and Solubility (13.2.3)

Vapor Pressure Lowering (13.3.1)

Boiling Point Elevation and Freezing Point Depression (13.3.2)

Boiling Point Elevation Problem (13.3.3)

Osmosis (13.3.4)

Colligative Properties of Ionic Solutions (13.3.5)

An Introduction to Reaction Rates (14.1.1)

Rate Laws: How the Reaction Rate Depends on Concentration (14.1.2)

Determining the Form of a Rate Law (14.1.3)

First-Order Reactions (14.2.1)

Second-Order Reactions (14.2.2)

A Kinetics Problem (14.2.3)

The Collision Model (14.3.1)

The Arrhenius Equation (14.3.2)

Using the Arrhenius Equation (14.3.3)

Defining the Molecularity of a Reaction (14.4.1)

Determining the Rate Laws of Elementary Reactions (14.4.2)

Calculating the Rate Laws of Multi-step Reactions (14.4.3)

Steady State Kinetics (14.4.4)

Catalysts and Types of Catalysts (14.5.1)

A Word About Laboratory Safety (14.5.2)

CIA Demonstration: Elephant Shot (14.5.3)

CIA Demonstration: The Cobalt(II)-Catalyzed Reaction of Potassium Sodium Tartrate (14.5.4)

CIA Demonstration: The Copper-Catalyzed Decomposition of Acetone (14.5.5)

The Concept of Equilibrium (15.1.1)

The Law of Mass Action and Types of Equilibrium (15.1.2)

Predicting the Direction of a Reaction (15.2.2)

Strategies for Solving Equilibrium Problems (15.2.3)

Le Châtelier's Principle (15.3.1)

The Effect of Changing Amounts on Equilibrium (15.3.2)

Solving Problems Far from Equilibrium (15.2.4)

An Equilibrium Problem Using the Quadratic Equation (15.2.5)

The Effects of Pressure and Volume on Equilibrium (15.3.3)

The Effects of Temperature and Catalysts on Equilibrium (15.3.4)

CIA Demonstration: NO2/N2O4 (15.3.5)

CIA Demonstration: Shifting the Equilibrium of FeSCN2+ (15.3.6)

Arrhenius/Brønsted-Lowry Definitions of Acids and Bases (16.1.1)

Hydronium, Hydroxide, and the pH Scale (16.1.2)

Strong Acids and Bases (16.2.1)

CIA Demonstration: Natural Acid-Base Indicators (16.2.2)

Weak Acids (16.2.3)

Weak Bases (16.2.4)

Lewis Acids and Bases (16.2.5)

Trends in Acid and Base Strengths (16.2.6)

Strong Acid-Strong Base and Weak Acid-Strong Base Reactions (17.1.1)

Strong Acid-Weak Base and Weak Acid-Weak Base Reactions (17.1.2)

The Common Ion Effect (17.1.3)

An Introduction to Buffers (17.2.1)

CIA Demonstration: Buffers in Action (17.2.2)

Acidic Buffers (17.2.3)

Basic Buffers (17.2.4)

The Henderson-Hasselbalch Equation (17.2.5)

Strong Acid-Strong Base Titration (17.3.1)

CIA Demonstration: Barium Hydroxide-Sulfuric Acid Titration (17.3.2)

Weak Acid-Strong Base Titration (17.3.3)

Polyprotic Acid-Strong Base Titration (17.3.4)

Weak Base-Strong Acid Titration (17.3.5)

Acid-Base Indicators (17.3.6)

The Solubility Product Constant (17.4.1)

CIA Demonstration: Silver Chloride and Ammonia (17.4.2)

Solubility and the Common Ion Effect (17.4.3)

Fractional Precipitation (17.4.4)

Spontaneous Processes (18.1.1)

Entropy and the Second Law of Thermodynamics (18.2.1)

Entropy and Temperature (18.2.2)

Gibbs Free Energy (18.3.1)

Standard Free Energy Changes of Formation (18.3.2)

Enthalpy and Entropy Contributions to K (18.4.1)

The Temperature Dependence of K (18.4.2)

Free Energy Away from Equilibrium (18.4.3)

Reviewing Oxidation-Reduction Reactions (19.1.1)

Electrochemical Cells (19.2.1)

Electromotive Force (19.2.2)

Standard Reduction Potentials (19.2.3)

Using Standard Reduction Potentials (19.2.4)

The Nernst Equation (19.2.5)

Electrochemical Determinants of Equilibria (19.2.6)

Batteries (19.3.1)

CIA Demonstration: The Fruit-Powered Clock (19.3.2)

Corrosion and the Prevention of Corrosion (19.4.1)

Electrolytic Cells (19.5.1)

The Stoichiometry of Electrolysis (19.5.2)

The Nature of Radioactivity (20.1.1)

The Stability of Atomic Nuclei (20.1.2)

Binding Energy (20.1.3)

Rates of Disintegration Reactions (20.2.1)

Radiochemical Dating (20.2.2)

Nuclear Fission (20.3.1)

Nuclear Fusion (20.3.2)

Applications of Nuclear Chemistry (20.3.3)

Metallurgical Processes (21.1.1)

The Band Theory of Conductivity (21.1.2)

Intrinsic Semiconductors (21.1.3)

Doped Semiconductors (21.1.4)

The Alkali Metals (21.2.1)

The Alkaline Earth Metals (21.2.2)

Aluminum (21.2.3)

CIA Demonstration: The Reaction Between Al and Br2 (21.2.4)

General Properties of Nonmetals (22.1.1)

Hydrogen (22.1.2)

General Properties of Carbon (22.2.1)

Silicon (22.2.2)

Nitrogen (22.3.1)

Phosphorus (22.3.2)

Oxygen (22.4.1)

CIA Demonstration: Creating Acid Rain (22.4.2)

Sulfur (22.4.3)

Halogens (22.5.1)

Aqueous Halogen Compounds (22.5.2)

Properties of Noble Gases (22.6.1)