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Stoichiometry: Converting Moles to Mass in Photosynthetic Reactions

Calculate the mass of carbon dioxide needed to react with 3.00 mol of H2O in a photosynthetic reaction. Use the molecular weights of the substances involved. Follow the steps to determine the required mass accurately.

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Stoichiometry: Converting Moles to Mass in Photosynthetic Reactions

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  1. Stoichiometry • Part 2b: moles to mass

  2. What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem?

  3. What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g)

  4. What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g)

  5. What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g)

  6. What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) ?

  7. What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) ? n (mol)

  8. What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) ? n (mol) 3.00

  9. What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) ? n (mol) 3.00

  10. 1 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) ? n (mol) 3.00

  11. 1 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) ? n (mol) 3.00

  12. 2 1 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) ? n (mol) 3.00

  13. 2 1 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) ? n (mol) 3.00 Step 1:

  14. 2 1 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) ? n (mol) 3.00 Step 1: Find the number of moles of CO2 used in the reaction.

  15. 2 1 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) ? n (mol) 3.00 Step 1: Find the number of moles of CO2 used in the reaction. nCO2/nH2O = coeffCO2/coeffH2O

  16. 2 1 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) ? n (mol) 3.00 Step 1: Find the number of moles of CO2 used in the reaction. nCO2/nH2O = coeffCO2/coeffH2O nCO2 = (nH2O)(coeffCO2)/coeffH2O

  17. 2 1 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) ? n (mol) 3.00 Step 1: Find the number of moles of CO2 used in the reaction. nCO2/nH2O = coeffCO2/coeffH2O nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6)

  18. 2 1 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) ? n (mol) 3.00 Step 1: Find the number of moles of CO2 used in the reaction. nCO2/nH2O = coeffCO2/coeffH2O nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 mol

  19. 2 1 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) ? n (mol) 3.00 Step 1: Find the number of moles of CO2 used in the reaction. nCO2/nH2O = coeffCO2/coeffH2O nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 mol

  20. 2 1 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) ? n (mol) 3.00 3.00 Step 1: Find the number of moles of CO2 used in the reaction. nCO2/nH2O = coeffCO2/coeffH2O nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 mol

  21. 2 1 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) ? n (mol) 3.00 3.00 Step 1: Find the number of moles of CO2 used in the reaction. nCO2/nH2O = coeffCO2/coeffH2O nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 mol

  22. 2 1 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) ? n (mol) 3.00 3.00 Step 1: Find the number of moles of CO2 used in the reaction. nCO2/nH2O = coeffCO2/coeffH2O nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 mol Step 2:

  23. 2 1 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) ? n (mol) 3.00 3.00 Step 1: Find the number of moles of CO2 used in the reaction. nCO2/nH2O = coeffCO2/coeffH2O nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 mol Step 2: Find the mass of the CO2 used in the reaction.

  24. 2 1 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) ? n (mol) 3.00 3.00 Step 1: Find the number of moles of CO2 used in the reaction. nCO2/nH2O = coeffCO2/coeffH2O nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 mol Step 2: Find the mass of the CO2 used in the reaction. mCO2 = (nCO2)(ṂCO2)

  25. 2 1 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) ? n (mol) 3.00 3.00 Step 1: Find the number of moles of CO2 used in the reaction. nCO2/nH2O = coeffCO2/coeffH2O nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 mol Step 2: Find the mass of the CO2 used in the reaction. mCO2 = (nCO2)(ṂCO2) = (3.00 mol)(44.0 g/mol)

  26. 2 1 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) ? n (mol) 3.00 3.00 Step 1: Find the number of moles of CO2 used in the reaction. nCO2/nH2O = coeffCO2/coeffH2O nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 mol Step 2: Find the mass of the CO2 used in the reaction. mCO2 = (nCO2)(ṂCO2) = (3.00 mol)(44.0 g/mol) = 132 g

  27. 2 1 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) ? n (mol) 3.00 3.00 Step 1: Find the number of moles of CO2 used in the reaction. nCO2/nH2O = coeffCO2/coeffH2O nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 mol Step 2: Find the mass of the CO2 used in the reaction. mCO2 = (nCO2)(ṂCO2) = (3.00 mol)(44.0 g/mol) = 132 g

  28. 2 1 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) 132 g n (mol) 3.00 3.00 Step 1: Find the number of moles of CO2 used in the reaction. nCO2/nH2O = coeffCO2/coeffH2O nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 mol Step 2: Find the mass of the CO2 used in the reaction. mCO2 = (nCO2)(ṂCO2) = (3.00 mol)(44.0 g/mol) = 132 g

  29. 2 1 What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) 132 g n (mol) 3.00 3.00 Step 1: Find the number of moles of CO2 used in the reaction. nCO2/nH2O = coeffCO2/coeffH2O nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 mol Step 2: Find the mass of the CO2 used in the reaction. mCO2 = (nCO2)(ṂCO2) = (3.00 mol)(44.0 g/mol) = 132 g

  30. What mass of carbon dioxide, in grams, is needed to react 3.00 mol of H2O in the photosynthetic reaction described in the previous problem? Ṃ (g/mol) 44.0 18.0 180.2 32.0 6 CO2(g) + 6 H2O(l) → C6H12O6(s) + 6 O2(g) m (g) 132 g n (mol) 3.00 3.00 Step 1: Find the number of moles of CO2 used in the reaction. nCO2/nH2O = coeffCO2/coeffH2O nCO2 = (nH2O)(coeffCO2)/coeffH2O = (3.00 mol)(6)/(6) = 3.00 mol Step 2: Find the mass of the CO2 used in the reaction. mCO2 = (nCO2)(ṂCO2) = (3.00 mol)(44.0 g/mol) = 132 g

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