1 / 16

Understanding Mole Conversions in Chemistry: Gas Volume, Mass and Particles

This tutorial focuses on mole conversions related to gases, including their volume, mass, and number of particles. By the end, you'll understand how to relate moles to gas volume at standard temperature and pressure (STP), convert between moles and mass, and calculate the number of particles. Through practice problems and examples, learn to apply Avogadro's Hypothesis and understand density effects for gases not at STP. Mastering these concepts is essential for solving complex chemistry problems and enhancing your scientific knowledge.

elana
Télécharger la présentation

Understanding Mole Conversions in Chemistry: Gas Volume, Mass and Particles

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Science 10H Chem Extra #2: Mole Conversions

  2. Objectives By the end of the lesson you should be able to: • Relate moles to the volume of a gas • Convert between moles, mass, # of particlesand volume of a gas • Convert using densities not at STP

  3. Avogadro’s Hypothesis Equal volumes of different gases, at the same temperature and pressure, contain the same number of particles • All gas samples with the same pressure, temperature and # of particles will occupy the same volume • STP: standard temperature and pressure (0oC and 101.3 kPa)

  4. STP • 1 mol of ANY GAS at STP has a volume of 22.4L • CONVERSION FACTOR: 1 mol or 22.4L 22.4L 1 mol

  5. Practice • What is the volume occupied by the following gases at STP: • 0.350 mol of SO2(g) • 12.5 mol of NH3 (g) • 0.350 mol of O2 (g) • 4.25 mol of HCl (g)

  6. Practice 2. Calculate the number of moles of the following gases at STP: • 10.0 L • 85.9 L of H2(g) • 375 mL of SO3 (g) • 5.00 mL of OCl2 (g)

  7. Recall… • CONVERSION FACTOR: 1mol or 6.02 X 1023molecules 6.02 X 1023molecules 1 mol Using the above conversion factor could we figure out how many molecules are in 0.125 mol of molecules? YEP we can!!! Let’s figure it out!! 

  8. More Practice….. • How many moles of N atoms are there in 5.00 x 1017 N atoms? • A light source emits 8.50 X 1017 photons per second. How many moles of photons are emitted by the light source in one minute? • A particular variety of C atom has a mass of 2.16 X 10-23 g/atom. What is the mass of a mole of this variety of C atom? Worksheet time!!

  9. Atoms and Molecules… • Before we can jump into more complex conversions we need to understand how to calculate how many atoms are in a molecule i.e. how many atoms are there in 5 molecules of CuSO4∙5H2O? Step 1: how many in one molecule? 21 Step 2: multiple it up! # of atoms = 5 molecules X 21 atoms = 105 atoms molecule

  10. Atoms and Molecules CONVERSION FACTOR: # atoms or 1 molecule. 1 Molecule # atoms

  11. Practice 1. Calculate how many atoms are contained in 3 molecules of each of the following: • CH3CO2H • NH4Cl • (CH3)2CO • (NH4)2SO4 • Ni(H2O)4(NH3)2Cl2

  12. Toughies!! • Up until now we have only done single stepper conversions (1 step conversions)….. • We must always convert from our given units into moles and then into our final units. • The MOLE is central to all conversions!! • Let’s use an overview to help!

  13. OVERVIEW! MASS OF A SUBSTANCE MOLAR MASS OF SUBSTANCE MOLES (of a substance) AVOGADRO’S NUMBER PARTICLES OF A SUBSTANCE MOLAR VOLUME VOLUME OF A SUBSTANCE

  14. Practice… • What is the volume occupied by 50.0 g of NH3 (g) at STP? • What is the mass of 1.00 X 1012 atoms of Cl? • How many oxygen atoms are contained in 75.0 L of SO3(g) at STP? Toughie Practice Time!

  15. DENSITY ISSUES! • So far we have only looked at gases at STP….but sometimes they aren’t going to be! • They will indicate this by including the density! • RECALL: d = m v

  16. Density examples: • What is the volume occupied by 3.00 mol of CH3CH2OH(l)? (d = 0.790 g/ml) • How many moles of Hg(l) are contained in 100 mL of Hg(l)? (d = 13.6 g/ml) • What is the density of O2 at STP? • A 2.50 L bulb contains 4.01g of a gas at STP. What is the molar mass of the gas? • Al2O3(s) has a density of 3.97 g/ml. How many atoms of Al are in 100 mL of Al2O3?

More Related