Multiple Choice
A 4.30 L gas has a pressure of 7.0 atm when the temperature is 60.0 ºC. What will be the temperature of the gas mixture if the volume and pressure are decreased to 2.45 L and 403.0 kPa respectively?
Table of contents
- 1. Matter and Measurements
- What is Chemistry?
- The Scientific Method
- Classification of Matter
- States of Matter
- Physical & Chemical Changes
- Chemical Properties
- Physical Properties
- Intensive vs. Extensive Properties
- Temperature (Simplified)
- Scientific Notation
- SI Units (Simplified)
- Metric Prefixes
- Significant Figures (Simplified)
- Significant Figures: Precision in Measurements
- Significant Figures: In Calculations
- Conversion Factors (Simplified)
- Dimensional Analysis
- Density
- Specific Gravity
- Density of Geometric Objects
- Density of Non-Geometric Objects
- 2. Atoms and the Periodic Table
- The Atom (Simplified)
- Subatomic Particles (Simplified)
- Isotopes
- Ions (Simplified)
- Atomic Mass (Simplified)
- Atomic Mass (Conceptual)
- Periodic Table: Element Symbols
- Periodic Table: Classifications
- Periodic Table: Group Names
- Periodic Table: Representative Elements & Transition Metals
- Periodic Table: Elemental Forms (Simplified)
- Periodic Table: Phases (Simplified)
- Law of Definite Proportions
- Atomic Theory
- Rutherford Gold Foil Experiment
- Wavelength and Frequency (Simplified)
- Electromagnetic Spectrum (Simplified)
- Bohr Model (Simplified)
- Emission Spectrum (Simplified)
- Electronic Structure
- Electronic Structure: Shells
- Electronic Structure: Subshells
- Electronic Structure: Orbitals
- Electronic Structure: Electron Spin
- Electronic Structure: Number of Electrons
- The Electron Configuration (Simplified)
- Electron Arrangements
- The Electron Configuration: Condensed
- The Electron Configuration: Exceptions (Simplified)
- Ions and the Octet Rule
- Ions and the Octet Rule (Simplified)
- Valence Electrons of Elements (Simplified)
- Lewis Dot Symbols (Simplified)
- Periodic Trend: Metallic Character
- Periodic Trend: Atomic Radius (Simplified)
- 3. Ionic Compounds
- Periodic Table: Main Group Element Charges
- Periodic Table: Transition Metal Charges
- Periodic Trend: Ionic Radius (Simplified)
- Periodic Trend: Ranking Ionic Radii
- Periodic Trend: Ionization Energy (Simplified)
- Periodic Trend: Electron Affinity (Simplified)
- Ionic Bonding
- Naming Monoatomic Cations
- Naming Monoatomic Anions
- Polyatomic Ions
- Naming Ionic Compounds
- Writing Formula Units of Ionic Compounds
- Naming Ionic Hydrates
- Naming Acids
- 4. Molecular Compounds
- Covalent Bonds
- Naming Binary Molecular Compounds
- Molecular Models
- Bonding Preferences
- Lewis Dot Structures: Neutral Compounds (Simplified)
- Multiple Bonds
- Multiple Bonds (Simplified)
- Lewis Dot Structures: Multiple Bonds
- Lewis Dot Structures: Ions (Simplified)
- Lewis Dot Structures: Exceptions (Simplified)
- Resonance Structures (Simplified)
- Valence Shell Electron Pair Repulsion Theory (Simplified)
- Electron Geometry (Simplified)
- Molecular Geometry (Simplified)
- Bond Angles (Simplified)
- Dipole Moment (Simplified)
- Molecular Polarity (Simplified)
- 5. Classification & Balancing of Chemical Reactions
- Chemical Reaction: Chemical Change
- Law of Conservation of Mass
- Balancing Chemical Equations (Simplified)
- Solubility Rules
- Molecular Equations
- Types of Chemical Reactions
- Complete Ionic Equations
- Calculate Oxidation Numbers
- Redox Reactions
- Spontaneous Redox Reactions
- Balancing Redox Reactions: Acidic Solutions
- Balancing Redox Reactions: Basic Solutions
- Balancing Redox Reactions (Simplified)
- Galvanic Cell (Simplified)
- 6. Chemical Reactions & Quantities
- 7. Energy, Rate and Equilibrium
- Nature of Energy
- First Law of Thermodynamics
- Endothermic & Exothermic Reactions
- Bond Energy
- Thermochemical Equations
- Heat Capacity
- Thermal Equilibrium (Simplified)
- Hess's Law
- Rate of Reaction
- Energy Diagrams
- Chemical Equilibrium
- The Equilibrium Constant
- Le Chatelier's Principle
- Solubility Product Constant (Ksp)
- Spontaneous Reaction
- Entropy (Simplified)
- Gibbs Free Energy (Simplified)
- 8. Gases, Liquids and Solids
- Pressure Units
- Kinetic Molecular Theory
- The Ideal Gas Law
- The Ideal Gas Law Derivations
- The Ideal Gas Law Applications
- Chemistry Gas Laws
- Chemistry Gas Laws: Combined Gas Law
- Standard Temperature and Pressure
- Dalton's Law: Partial Pressure (Simplified)
- Gas Stoichiometry
- Intermolecular Forces (Simplified)
- Intermolecular Forces and Physical Properties
- Atomic, Ionic and Molecular Solids
- Heating and Cooling Curves
- 9. Solutions
- Solutions
- Solubility and Intermolecular Forces
- Solutions: Mass Percent
- Percent Concentrations
- Molarity
- Osmolarity
- Parts per Million (ppm)
- Solubility: Temperature Effect
- Intro to Henry's Law
- Henry's Law Calculations
- Dilutions
- Solution Stoichiometry
- Electrolytes (Simplified)
- Equivalents
- Molality
- The Colligative Properties
- Boiling Point Elevation
- Freezing Point Depression
- Osmosis
- Osmotic Pressure
- 10. Acids and Bases
- Acid-Base Introduction
- Arrhenius Acid and Base
- Bronsted Lowry Acid and Base
- Acid and Base Strength
- Ka and Kb
- The pH Scale
- Auto-Ionization
- pH of Strong Acids and Bases
- Acid-Base Equivalents
- Acid-Base Reactions
- Gas Evolution Equations (Simplified)
- Ionic Salts (Simplified)
- Buffers
- Henderson-Hasselbalch Equation
- Strong Acid Strong Base Titrations (Simplified)
- 11. Nuclear Chemistry
- BONUS: Lab Techniques and Procedures
- BONUS: Mathematical Operations and Functions
- 12. Introduction to Organic Chemistry
- 13. Alkenes, Alkynes, and Aromatic Compounds
- 14. Compounds with Oxygen or Sulfur
- 15. Aldehydes and Ketones
- 16. Carboxylic Acids and Their Derivatives
- 17. Amines
- 18. Amino Acids and Proteins
- 19. Enzymes
- 20. Carbohydrates
- Intro to Carbohydrates
- Classification of Carbohydrates
- Fischer Projections
- Enantiomers vs Diastereomers
- D vs L Enantiomers
- Cyclic Hemiacetals
- Intro to Haworth Projections
- Cyclic Structures of Monosaccharides
- Mutarotation
- Reduction of Monosaccharides
- Oxidation of Monosaccharides
- Glycosidic Linkage
- Disaccharides
- Polysaccharides
- 21. The Generation of Biochemical Energy
- 22. Carbohydrate Metabolism
- 23. Lipids
- 24. Lipid Metabolism
- 25. Protein and Amino Acid Metabolism
- 26. Nucleic Acids and Protein Synthesis
- Intro to Nucleic Acids
- Nitrogenous Bases
- Nucleoside and Nucleotide Formation
- Naming Nucleosides and Nucleotides
- Phosphodiester Bond Formation
- Primary Structure of Nucleic Acids
- Base Pairing
- DNA Double Helix
- Intro to DNA Replication
- Steps of DNA Replication
- Types of RNA
- Overview of Protein Synthesis
- Transcription: mRNA Synthesis
- Processing of pre-mRNA
- The Genetic Code
- Introduction to Translation
- Translation: Protein Synthesis
8. Gases, Liquids and Solids
Chemistry Gas Laws: Combined Gas Law
Back8. Gases, Liquids and Solids
Chemistry Gas Laws: Combined Gas Law
- Multiple Choice
A sealed container with a movable piston contains a gas with a pressure of 1380 torr, a volume of 820 mL and a temperature of 31°C. What would the volume be if the new pressure is now 2.83 atm, while the temperature decreased to 25°C?
- Open QuestionRearrange the variables in the combined gas law to solve for P₂
- Open QuestionA sample of argon gas has a volume of 735 mL at a pressure of 1.20 atm and a temperature of 112 °C. What is the final volume of the gas, in milliliters, when the pressure and temperature of the gas sample are changed to the following, ifthe amount of gas does not change?a. 658 mmHg and 281 K