1 / 13

Gases and Stoichiometry

Gases and Stoichiometry. Review Ideal Gas Law Gas Law Stoichiometry. Ideal Gas Law. Remember, mathematically, PV=nRT Where R = 8.31 LkPa/molK. Pressure x vol. = # of moles x ideal gas constant x temp. Ideal Gas Law.

steel-joseph
Download Presentation

Gases and Stoichiometry

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. Gases and Stoichiometry Review Ideal Gas Law Gas Law Stoichiometry

  2. Ideal Gas Law • Remember, mathematically, PV=nRT • Where R = 8.31 LkPa/molK Pressure x vol. = # of moles x ideal gas constant x temp.

  3. Ideal Gas Law • Now that we have talked more exhaustively about the subject of moles as it relates to mass, we can add a new type of problem.

  4. Practice Problem • What volume will 12 grams of oxygen gas (O2) will occupy at 25oC and 52.7 kPa?

  5. Practice Problem • How many grams of carbon dioxide can be contained in a 17.8L container at 22oC and 188kPa?

  6. Gas Stoichiometry • Remember when we looked at chemical quantities and said that for any gas, 1 mole = 22.4L @ STP? • Now we know that if you change the temperature and pressure, the relationship doesn’t work!

  7. Gas Law Stoichiometry • If gases are being produced or consumed in a chemical reaction, we can use stoichiometry along with the ideal gas law to solve problems for gases NOT at standard temperature and pressure.

  8. Practice Problem • In the reaction KClO3 KCl + O2 38.5g of potassium chlorate are burned and the resultant oxygen is captured at 100.7kPa and 298K. What volume of oxygen is generated?

  9. Practice Problem • In the combustion of 25.3g methane (CH4), the carbon dioxide produced is trapped in a 31.3L container at 31oC. What is the pressure due to carbon dioxide in this container? (remember to write a balanced equation)

  10. Molarity Review • Remember, molarity is the SI measure of concentration, found by taking the number of moles solute per liter of solution. M = (mol solute)/(L solution)

  11. Now that we have talked more exhaustively about the subject of moles as it relates to mass, we can use it with concentration.

  12. Practice Problem • What is the molarity of a solution made by adding 38.77g MgSO4 to enough water to make 0.85L solution?

  13. Practice Problem • How many grams of sodium nitrate are needed to make 500mL of 2.0M solution?

More Related