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Chemistry: A Molecular Approach, 1 st Edition Nivaldo J. Tro

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  1. Chemistry: A Molecular Approach, 1st Edition Nivaldo J. Tro Chapter 4 Chemical Quantities and Aqueous Reactions

  2. The overall equation involved in photosynthesis is: 6 CO2 + 6 H2O  2 C6H12O6 + 6 O2 How many grams of glucose (C6H12O6) form when 4.40 g of CO2 react? • 18.0 g • 3.00 g • 108 g • 0.0167 g Tro Chemistry: A Molecular Approach

  3. The overall equation involved in photosynthesis is: 6 CO2 + 6 H2O  2 C6H12O6 + 6 O2 How many grams of glucose (C6H12O6) form when 4.40 g of CO2 react? • 18.0 g • 3.00 g • 108 g • 0.0167 g Tro Chemistry: A Molecular Approach

  4. The rapid decomposition of sodium azide, NaN3, to its elements is one of the reactions used to inflate airbags: 2 NaN3 (s)  2 Na (s) + 3 N2 (g) How many grams of N2 are produced from 6.00 g of NaN3 N2 Na • 3.88 g • 1.72 g • 0.138 g • 2.59 g Tro Chemistry: A Molecular Approach

  5. The rapid decomposition of sodium azide, NaN3, to its elements is one of the reactions used to inflate airbags: 2 NaN3 (s)  2 Na (s) + 3 N2 (g) How many grams of N2 are produced from 6.00 g of NaN3 N2 Na • 3.88 g • 1.72 g • 0.138 g • 2.59 g Tro Chemistry: A Molecular Approach

  6. Ammonia is produced using the Haber process: 3 H2 + N2 2 NH3 What mass of ammonia could be produced from 15.0 kg each of H2 and N2? Assume the reaction goes to completion. • 18.2 g • 9.11g • 1.82 x 104 g • 9.11x 103 g • 8.45 x 104 g Tro Chemistry: A Molecular Approach

  7. Ammonia is produced using the Haber process: 3 H2 + N2 2 NH3 What mass of ammonia could be produced from 15.0 kg each of H2 and N2? Assume the reaction goes to completion. • 18.2 g • 9.11g • 1.82 x 104 g • 9.11x 103 g • 8.45 x 104 g Tro Chemistry: A Molecular Approach

  8. What mass, in grams, of sodium bicarbonate, NaHCO3, is required to neutralize 1000.0 L of 0.350 M H2SO4? • 2.94 x 104 • 1.47 x 104 • 5.88 x 104 • 3.50 x 103 • 1.75 x 103 • 7.00 x 103 Tro Chemistry: A Molecular Approach

  9. What mass, in grams, of sodium bicarbonate, NaHCO3, is required to neutralize 1000.0 L of 0.350 M H2SO4? • 2.94 x 104 • 1.47 x 104 • 5.88 x 104 • 3.50 x 103 • 1.75 x 103 • 7.00 x 103 Tro Chemistry: A Molecular Approach

  10. Aqueous solutions of which of the following would conduct electricity? • AgNO3 • C11H22O11 (sucrose: table sugar) • CH3CH2OH (ethanol) • O2 • All of the above • None of the above Tro Chemistry: A Molecular Approach

  11. Aqueous solutions of which of the following would conduct electricity? • AgNO3 • C11H22O11 (sucrose: table sugar) • CH3CH2OH (ethanol) • O2 • All of the above • None of the above Tro Chemistry: A Molecular Approach

  12. Sulfuric acid is found in some types of batteries. What volume of 3.50 M H2SO4 is required to prepare 250.0 mL of 1.25 M H2SO4? • 17.5 mL • 700. mL • 89.3 mL • 109 mL • None of the above Tro Chemistry: A Molecular Approach

  13. Sulfuric acid is found in some types of batteries. What volume of 3.50 M H2SO4 is required to prepare 250.0 mL of 1.25 M H2SO4? • 17.5 mL • 700. mL • 89.3 mL • 109 mL • None of the above Tro Chemistry: A Molecular Approach

  14. H2PO4–SO32–N2O4 Determine the oxidation number of the red element in each of the following compounds: • + 6 + 6 + 4 • + 5 + 2 + 4 • + 5 + 4 + 4 • + 5 + 4 + 8 • + 6 + 4 + 4 Tro Chemistry: A Molecular Approach

  15. H2PO4–SO32–N2O4 Determine the oxidation number of the red element in each of the following compounds: • + 6 + 6 + 4 • + 5 + 2 + 4 • + 5 + 4 + 4 • + 5 + 4 + 8 • + 6 + 4 + 4 Tro Chemistry: A Molecular Approach