Moles and the Avogadro constant

Slides:



Advertisements
Similar presentations
Moles, volume and density
Advertisements

Title: Lesson 8: Calculations involving Volumes of Gases Learning Objectives: Understand that a fixed quantity (in moles) of gas, always occupies the same.
COMBINED GAS LAW AND AVOGADRO’S PRINCIPLE. COMBINED GAS LAW P1V1P2V2T1T2P1V1P2V2T1T2 =
The Mole–Mass Relationship How do you convert the mass of a substance to the number of moles of the substance? 10.2.
Chemical Quantities.  Calculate the mass of compounds.  Calculate the molar volumes of gases.  Solve problems requiring conversions between mass, and.
Mullis1 Gay Lussac’s law of combining volumes of gases When gases combine, they combine in simple whole number ratios. These simple numbers are the coefficients.
Topic 10 Gases III. Ideal Gas Law.
Relating Mass to Numbers of Atoms The mole, Avogadro’s number, and molar mass provide the basis for relating masses in grams to moles.
Calculate the amount of substance in moles, using gas volumes
Gas Stoichiometry Non-Standard Conditions. The relationship between volume and moles (n)
Gas Stoichiometry!. equal volumes of gases at the same temperature & pressure contain equal numbers of particles equal volumes of gases at the same temperature.
Chapter 14-3 I. Avogadro’s Principle A. Equal volumes of gases at same T and P contain equal #’s of molecules B. H 2 + Cl 2 → 2HCl 1 vol. 1 vol. 2 vol.
Chapter 14-3 I. Avogadro’s Principle A. Equal volumes of gases at same T and P contain equal #’s of molecules B. H 2 + Cl 2 → 2HCl 1 vol. 1 vol. 2 vol.
3.4Molar Volume Molar Volume The Molar Volume of Gases Multi-Step Conversions Involving the Volume of a Substance Molar Volume and Density.
Ideal Gas Law.
Ideal gases and molar volume
Avogadro’s law Equal volumes of different gases at the same temperature and pressure have the same number of moles. Example: Cl2 (g) + H2 (g)
Unit 1 Gases. Ideal Gases Objectives 1. Compute the value of an unknown using the ideal gas law. 2. Compare and contrast real and ideal gases.
UNIT 6: CHEMICAL QUANTITIES Chapter 10: Mole and Volume Relationships.
Avogadro's Principle “Equal volumes of gases at the same temperature and pressure contain equal numbers of particles” It doesn’t matter what type of gas.
Miss Fogg Spring 2016  A particle can refer to an individual atom OR a type of molecule ◦ Jellybean ◦ Baseball ◦ Carbon atoms ◦ Hydrogen atoms ◦ Water.
Gas volumes and moles PAGE 87 OF INB. Essential Question:  How can 2 liters of Hydrogen react with 1 liter of Oxygen and only produce 2 liters of gas?
Gas Laws Kinetic Theory assumptions Gas particles do not attract or repel Small particles in constant random motion Elastic collisions All gases have the.
What is a mole? A mole is a number. It is x This number is also called Avogadro’s number. How many atoms in 1 mole of copper atoms?
IB1 Chemistry Quantitative chemistry Apply the concept of molar volume at standard temperature and pressure in calculations Solve problems.
Gas Laws. GAS LAWS They’ll save your life! Boyle’s Law Charles’s Law Lussac’s Law Avogadro’s Law –Molar Volume Combined Gas Law Ideal Gas Law.
The Gas Laws Chemistry Dr. May.
Gases.
Chapter 12 Notes, Part II Ideal Gas Law
Molar Mass and Molar Volume
Ideal Gas Law (p ) please read the text first
Thermal Properties of Matter
Ch. 10 Chemical Quantities
The Mole.
The Ideal Gas Law.
Quantitative chemistry
The Gas Laws Chemistry Dr. May.
Ideal Gas Law PV=nRT.
Mole-Mass and Mole-Volume Relationships
Warmup Mg(s) + 2 HCl(g)  MgCl2 (aq) + H2 (g))
Ch. 11: Molecular Composition of Gases
Gas Volumes and the Ideal Gas Law
3.3 The Molar Volume Pages
Ch. 10 & 11 - Gases III. Ideal Gas Law (p , )
11.8 Tro's Introductory Chemistry, Chapter 11.
Avogadro’s Law.
Topic 10 Gases III. Ideal Gas Law.
Ch. 13 Gases III. Ideal Gas Law (p ).
Ch. 10 & 11 - Gases III. Ideal Gas Law (p , )
Chapter 19 Avogadro’s Principle.
Avogadro’s Law.
III. Ideal Gas Law (p , in class)
Moles and Gas Volume (3.4) Avogadro’s Hypothesis: equal volumes of different gases at the same temperature and pressure contain the same number of particles.
Moles, Volume and Density
The Mole.
Molar Volume.
Section 3 Gas Volumes and the Ideal Gas Law
III. Ideal Gas Law (p , in class)
Gas Volumes and Ideal Gas Law
Lesson 5.4 – Ideal Gases Chemistry 1 Honors Dr. J. Venables
Chapter 12 Notes, Part II Ideal Gas Law
The Combined Gas Law and Avogadro’s Principle
Chapter 10: Chemical Quantities Mole – Volume Relationships
Presentation transcript:

Moles and the Avogadro constant Boardworks A2 Physics Thermal Physics Teacher notes It may be worth pointing out to students that, unlike most measurements which take explicit units (grams, millilitres), the mole is a dimensionless quantity that simply converts very large numbers of particles into more manageable sizes.

Avogadro’s law Boardworks A2 Physics Thermal Physics In 1811 the Italian scientist Amedeo Avogadro developed a theory about the volume of gases. Avogadro’s law states that equal volumes of different gases at the same pressure and temperature will contain equal numbers of particles. For example, if there are 2 moles of O2 in 50 cm3 of oxygen gas, then there will be 2 moles of N2 in 50 cm3 of nitrogen gas and 2 moles of CO2 in 50 cm3 of carbon dioxide gas at the same temperature and pressure. Using this principle, the volume that a gas occupies will depend on the number of moles of the gas.

Molar volumes of gases Boardworks A2 Physics Thermal Physics If the temperature and pressure are fixed at convenient standard values, the molar volume of a gas can be determined. At standard temperature and pressure (273 K and 100 kPa), 1 mole of any gas occupies a volume of 2.24 × 10-2 m3. This is the molar volume. Example: What volume does 5 moles of CO2 occupy at standard temperature and pressure? volume occupied = no. moles × molar volume Teacher notes The definition of standard temperature and pressure varies from source to source. The most recent IUPAC (International Union of Pure and Applied Chemistry) definition is 273 K / 100 kPa, although its old definition was 273 K / 101 kPa. Other common definitions include 293 K / 101 kPa (the National Institute of Standards and Technology (NIST)). At 25°C / 100 kPa, the molar volume of an ideal gas is 2.48 × 10-2 m3. Molar volume is sometimes expressed in dm3, where 1 dm3 = 0.001 m3. These units are generally used by chemists. = 5 × (2.24 × 10-2) = 0.112 m3