1 / 14

Chapter 5 Chemical Reactions and Quantities

Chapter 5 Chemical Reactions and Quantities. 5.8 Mass Calculations for Reactions. Steps in Finding the Moles and Masses in a Chemical Reaction. Moles to Grams. Suppose we want to determine the mass (g) of NH 3 that can form from 2.50 moles N 2 .

wilbur
Télécharger la présentation

Chapter 5 Chemical Reactions and Quantities

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. Chapter 5 Chemical Reactions and Quantities 5.8 Mass Calculations for Reactions

  2. Steps in Finding the Moles and Masses in a Chemical Reaction

  3. Moles to Grams Suppose we want to determine the mass (g) of NH3 that can form from 2.50 moles N2. N2(g) + 3 H2(g) 2 NH3(g) The plan needed would be moles N2 moles NH3 grams NH3 The factors needed would be: mole factor NH3/N2and the molar mass NH3

  4. Moles to Grams The setup for the solution would be: 2.50 mole N2 x 2 moles NH3 x 17.0 g NH3 1 mole N2 1 mole NH3 given mole-mole factor molar mass = 85.0 g NH3

  5. Learning Check How many grams of O2 are needed to produce 0.400 mole Fe2O3 in the following reaction? 4 Fe(s) + 3 O2(g) 2 Fe2O3(s) 1) 38.4 g O2 2) 19.2 g O2 3) 1.90 g O2

  6. Solution 2) 19.2 g O2 0.400 mole Fe2O3 x 3 mole O2 x 32.0 g O2= 19.2 g O2 2 mole Fe2O3 1 mole O2 mole factor molar mass

  7. Calculating the Mass of a Reactant The reaction between H2 and O2 produces 13.1 g water. How many grams of O2 reacted? 2 H2(g) + O2(g) 2 H2O(g) ? g 13.1 g The plan and factors would be g H2O mole H2O mole O2 g O2 molar mole-mole molar mass H2O factor mass O2

  8. Calculating the Mass of a Reactant The setup would be: 13.1 g H2O x 1 mole H2O x 1 mole O2 x 32.0 g O2 18.0 g H2O 2 moles H2O 1 mole O2 molar mole-mole molar mass H2O factor mass O2 = 11.6 g O2

  9. Learning Check Acetylene gas C2H2 burns in the oxyacetylene torch for welding. How many grams of C2H2 are burned if the reaction produces 75.0 g CO2? 2 C2H2(g) + 5 O2(g) 4 CO2(g) + 2 H2O(g) 1) 88.6 g C2H2 2) 44.3 g C2H2 3) 22.2 g C2H2

  10. Solution 3) 22.2 g C2H2 2 C2H2(g) + 5 O2(g)4 CO2(g) + 2 H2O(g) 75.0 g CO2 x 1 mole CO2 x 2 moles C2H2 x 26.0 g C2H2 44.0 g CO2 4 moles CO2 1 mole C2H2 molar mole-mole molar mass CO2 factor mass C2H2 = 22.2 g C2H2

  11. Calculating the Mass of Product When 18.6 g ethane gas C2H6 burns in oxygen, how many grams of CO2 are produced? 2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(g) 18.6 g ? g The plan and factors would be g C2H6 mole C2H6 mole CO2 g CO2 molar mole-mole molar mass C2H6 factor mass CO2

  12. Calculating the Mass of Product 2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(g) The setup would be 18.6 g C2H6 x 1 mole C2H6 x 4 moles CO2 x 44.0 g CO2 30.1 g C2H6 2 moles C2H6 1 mole CO2 molar mole-mole molar mass C2H6 factor mass CO2 = 54.4 g CO2

  13. Learning Check How many grams H2O are produced when 35.8 g C3H8 react by the following equation? C3H8(g) + 5 O2(g) 3 CO2(g) + 4 H2O(g) 1) 14.6 g H2O 2) 58.4 g H2O 3) 117 g H2O

  14. Solution 2) 58.4 g H2O C3H8(g) + 5 O2(g) 3 CO2(g) + 4 H2O(g) 35.8 g C3H8x 1 mole C3H8 x 4 mole H2O x 18.0 g H2O 44.1 g C3H8 1 mole C3H8 1 mole H2O molar mole-mole molar mass C3H8 factor mass H2O = 58.4 g H2O

More Related