1 / 15

Practice with Molar Mass Problems

Practice with Molar Mass Problems. x 1 mol H 2. 2.02 g H 2. : Question #1. How many moles of H 2 are in 100 g of H 2 ?. # mol H 2. = 100 g H 2. = 49.5 mol H 2. x 1 mol CuSO 4. 159.61 g CuSO 4. Question #2.

Download Presentation

Practice with Molar Mass Problems

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. Practice with Molar Mass Problems

  2. x 1 mol H2 2.02 g H2 :Question #1 How many moles of H2 are in 100 g of H2? # mol H2 = 100 g H2 = 49.5 mol H2

  3. x 1 mol CuSO4 159.61 g CuSO4 Question #2 300 g of CuSO4 is needed in an experiment. How many moles does this represent? # mol CuSO4 = 300 g CuSO4 = 1.88 mol CuSO4

  4. x 143.32 g AgCl 1 mol AgCl Question #3 A chemical reaction requires 23.78 moles of silver chloride. How many grams is this? # g AgCl = 23.78 mol AgCl = 3408 g AgCl

  5. x 6.02x1023 molecules 1 mol H2O x 1 mol H2O 18.02 g H2O Question #4 How many molecules are in 73 grams H2O? # H2O molecules = 73 g H2O = 2.4 x 1024 molecules H2O

  6. x 1 mol Ca3(PO4)2 310.18 g Ca3(PO4)2 Question #5 255 g of calcium phosphate are produced in a chemical reaction. How many moles of calcium phosphate does this represent? # mol Ca3(PO4)2 = 255 g Ca3(PO4)2 = 0.822 mol Ca3(PO4)2

  7. 2 mol H2O 18.01 g H2O 265 g H2O x x = 1 mol O2 1 mol H2O Question #6 According to the equation 2H2 + O2 2H2O, how many grams of H2O would be produced if 7.35 mol of O2 is used up? (hint: you will need two conversion factors – 1 from the balanced equation and 1 from a molar mass) # g H2O= 7.35 mol O2

  8. And you thought Chemistry was bad with factor-label problems!!??

  9. Complete the following chart (#7 - #13):

  10. Formula Molar mass (g/mol) Mass (g) Moles (mol) Complete the following chart (answers): FeSO4 151.9 500 3.29 (NH4)2CO3 96.1 192.2 2 SnO2 150.7 50 0.332 Sb2O5 323.6 80.9 0.25 NaClO4 122.4 100 0.817 Mg(IO3)2 374.1 1196.8 3.2 CoCl2.H2O 147.8 332 2.246

  11. Assignment 14. AgCl = 143.35 g/mol #g = 2 mol x 143.35 g/mol =286.7 g (2) 15. H2 = 2.016 g/mol #mol = 100 g x mol/2.016 g =49.6 mol (2) 16. CuSO4 = 159.62 g/mol #mol= 300 g x mol/159.62 g =1.879 mol (2) 17. KClO = 90.55 g/mol #mol = 250 g x mol/90.55 g =2.76 mol (2)

  12. x 6.02x1023 molecules 1 mol H2O x 1 mol H2O 18.02 g H2O Extra Review Mass-Mole-Molecules: Determine the number of molecules in 73 g of water # H2O molecules = 73 g H2O = 2.4 x 1024 molecules H2O

  13. x 253.80 g I2 1 mol I2 x 3 mol I2 2 mol Al Try this one: Calculate the mass in grams of iodine required to react completely with 0.50 moles of aluminum. Al + I2 AlI3 2Al + 3 I2 2 AlI3 0.50 mol Al = 190 g I2

  14. x 253.80 g I2 1 mol I2 x 3 mol I2 x 1 mol Al 2 mol Al 26.98 g Al Try this one: Calculate the mass in grams of iodine required to react completely with 0.50 g of aluminum. Al + I2 AlI3 2Al + 3 I2 2 AlI3 0.50 g Al = 7.1 g I2

More Related