Universal Gas Equation - VCE Chemistry

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universal gas equation

VCE CHEMISTRY PREVIOUS STUDY DESIGN- 2016

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- Water >
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  - Precipitation reactions
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- Acids and Bases >
  - What are acids and bases?
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  - Dilution and reaction of acids
- Redox reactions >
  - What are redox reactions?
  - Oxidation numbers
  - Metal reactivity and half equations
  - Corrosion
- Analysis for salts in water >
  - Salts in water and mass/mass stoichiometry
  - Gravimetric analysis
  - Limiting and excess reagents
  - Colorimetry and UV/visible spectroscopy
  - AES and AAS
- Analysis of organic compounds in water >
  - Chromatography-paper and TLC
  - Chromatography- Column/HPLC
- Analysis of acids and bases in water >
  - Sources of acids and bases found in water
  - Acid/base calculations
  - Volumetric analysis
Unit 3
- Fuels >
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  - Chemical Energy
  - Energy profile diagrams
  - Heat of combustion
- Combustion of fuels >
  - Gases
  - Universal gas equation
  - Gas stoichiometry
- Redox reactions >
  - Redox Review
  - Oxidation numbers review
  - Review Metal reactivity and half equations
  - Complex redox reactions
- Galvanic cells >
  - What are galvanic cells?
  - Spontaneous reactions
  - Primary and secondary cells
- Fuel cells
- Electrolysis >
  - What is Electrolysis?
  - Industrial production- electrolysis
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- Rate of chemical reactions >
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Unit 4
- Organic compounds >
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  - Reactions of alkanes and alkenes
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- Analysis of organic compounds-IR, NMR and MS >
  - IR
  - NMR
  - Mass Spectroscopy
  - Combining techniques
- Analysis of organic compounds- Chromatography, HPLC >
  - Chromatography-paper and TLC
  - Chromatography- Column/HPLC
- Analysis of organic compounds- volumetric analysis >
  - Volumetric analysis
  - Organic acids and bases
- Structure and bonding of food molecules >
  - Fats and oils
  - Carbohydrates
  - Proteins
  - Vitamins
- Metabolism of food in the human body >
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  - Food metabolism
- The energy content of food >
  - Energy sources
  - Measuring energy
Exam question links
Scientific Reports and Posters
Study score
Chemistry basics
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STUDY CARD AVAILABLE- SEE CONTACT. Relationship between Pressure- Volume (Boyle's Law)•The volume of a fixed mass of gas at constant temperature is inversely proportional to the pressure exerted on it.•P ∞ 1 / V then PV equals a constant value.•Boyle’s Law: P1V1 = P2V2 at constant temperature.Relationship between Temperature- Volume (Charles' Law)•The volume of a fixed mass of gas at constant pressure is directly proportional to its absolute temperature (kelvin scale).•V ∞ T then V / T equals a constant value.•Charles’ Law: V1 = V2 at constant pressure T1 T2Relationship between Volume-Mole (Avogadro's Law)Avogadro postulated that equal volumes of gases at the same temperature and pressure contain equal numbers of particles. V ∞ n or V= kn where k is a constant.Molar gas Volume•Molar Gas Volume is the volume of 1 mole of a particular gas.•It has been found experimentally that 1 mole of any gas at STP occupies a volume of 22.7 L.•The molar volume of a gas at SLC is 24.8 L.•Gas constants: VSTP = 22.7 L VSLC = 24.8 LSTP- 0 oC and 100kPaSLC – 25 oC and 100KPaThere is a direct relationship between the number of moles of a gas and its molar volume. n = V VmWhere: n is the number of moles of gas V is the actual volume of gas Vm is the molar volume of the gas•Combine Boyle’s and Charles’ Laws: PV equals a constant value V / T equals a constant value to get PV / T equals a constant value.•Combined Gas Law: P1V1 = P2V2 for a constant amount of gas. T1 T2•P ∞ 1 / V (Boyle’s Law)•P ∞ T (Gay Lussac’s Law)•P ∞ n•Combine these proportionalities: P ∞ nT / VUniversal gas equation•Replace proportionality with equality sign.•Introduce a general gas constant, R and we get the general gas equation. PV = nRT where: Pressure (P) is measured in kilopascals (kPa) Volume (V) is measured in litres (L) Temperature (T) is measured in kelvin (K) Number of moles (n) – unit (mol) General Gas Constant (R) = 8.31JK-1mol-1 Aus-e-tute ideal gas law Ideal gas equation quiz Kahoot quiz- gas laws Ideal gas equation quiz Boyles law Charle's law Combined gas law

Boyle's Law animation courtesy of By NASA's Glenn Research Center - http://www.grc.nasa.gov/WWW/K-12/airplane/aboyle.html, Public Domain, https://commons.wikimedia.org/w/index.php?curid=4448761

Charle's Law animation courtesy of By NASA's Glenn Research Center - http://www.grc.nasa.gov/WWW/K-12/airplane/aglussac.html, Public Domain, https://commons.wikimedia.org/w/index.php?curid=4448734 Sample Problem using the universal gas equation Find the volume of 6.30 mol of carbon dioxide gas at 23oC and 550 kPa pressure. (R = 8.31 JK-1mol-1)Solution:Step 1: Write down given data in correct units. P = 550 kPa V = ??? n = 6.30 mol T = 23oC = 296 K R = 8.31 JK-1mol-1Step 2: Use general gas equation to calculate volume. PV = nRT V = nRT / P = 6.30 x 8.31 x 296 / 550 = 28.2 L

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Home
Unit 1
- Atomic theory >
  - Inside the atom
  - Electron configuration
  - Nanoparticles
  - Quiz
- The Periodic table >
  - History of the periodic table
  - Modern Periodic table
  - Periodic table trends
- Metals >
  - Properties of Metals
  - Metal reactivity
  - Alloys and extraction of metals
- Ionic bonding >
  - The ionic bond
  - Ionic bonding and formula writing
- Atomic mass and the mole >
  - Atomic mass
  - The Mole
  - Empirical and molecular formula
- Covalent bonding >
  - Properties and bonding
  - VSEPR THEORY
  - Polar and Non polar molecules
  - Intermolecular bonding
  - Carbon lattices
- Organic chemistry >
  - Hydrocarbons
  - Alkanes, alkenes and alkynes
  - Naming organic compounds
  - Functional groups
- Polymers >
  - Types of polymers
  - Polymer properties
  - Revision Unit 1
Unit 2
- Water >
  - Reactions of life
  - Properties of water
  - Heat capacity
  - Latent heat
- Solutions >
  - Water as a solvent
  - Solubility and dissolving
  - Precipitation reactions
  - Solubility curves
  - Concentration
- Acids and Bases >
  - What are acids and bases?
  - Strength of acids and bases
  - pH
  - Dilution and reaction of acids
- Redox reactions >
  - What are redox reactions?
  - Oxidation numbers
  - Metal reactivity and half equations
  - Corrosion
- Analysis for salts in water >
  - Salts in water and mass/mass stoichiometry
  - Gravimetric analysis
  - Limiting and excess reagents
  - Colorimetry and UV/visible spectroscopy
  - AES and AAS
- Analysis of organic compounds in water >
  - Chromatography-paper and TLC
  - Chromatography- Column/HPLC
- Analysis of acids and bases in water >
  - Sources of acids and bases found in water
  - Acid/base calculations
  - Volumetric analysis
Unit 3
- Fuels >
  - Types of fuels
  - Fossil fuels vs biofuels
- Using the energy from fuels >
  - Chemical Energy
  - Energy profile diagrams
  - Heat of combustion
- Combustion of fuels >
  - Gases
  - Universal gas equation
  - Gas stoichiometry
- Redox reactions >
  - Redox Review
  - Oxidation numbers review
  - Review Metal reactivity and half equations
  - Complex redox reactions
- Galvanic cells >
  - What are galvanic cells?
  - Spontaneous reactions
  - Primary and secondary cells
- Fuel cells
- Electrolysis >
  - What is Electrolysis?
  - Industrial production- electrolysis
  - Faraday's Laws
- Rate of chemical reactions >
  - Collision theory
  - Reaction rate
- Equilibrium >
  - What is equilibrium?
  - Le Chatelier's Principle
- Tests and useful websites
Unit 4
- Organic compounds >
  - Organic chemistry - review
  - Stereoisomers
  - More on functional groups
- Reactions of organic compounds >
  - Properties of organic compounds
  - Reactions of alkanes and alkenes
  - Reactions with functional groups
  - Reaction pathways
- Analysis of organic compounds-IR, NMR and MS >
  - IR
  - NMR
  - Mass Spectroscopy
  - Combining techniques
- Analysis of organic compounds- Chromatography, HPLC >
  - Chromatography-paper and TLC
  - Chromatography- Column/HPLC
- Analysis of organic compounds- volumetric analysis >
  - Volumetric analysis
  - Organic acids and bases
- Structure and bonding of food molecules >
  - Fats and oils
  - Carbohydrates
  - Proteins
  - Vitamins
- Metabolism of food in the human body >
  - Enzymes
  - Food metabolism
- The energy content of food >
  - Energy sources
  - Measuring energy
Exam question links
Scientific Reports and Posters
Study score
Chemistry basics
Contact
Remote learning
- Unit 1 resources
- Unit 2 resources
- Unit 3 resources
- Unit 4 resources

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