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5 moles 3/5 moles 15 moles 3 moles PowerPoint Presentation
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5 moles 3/5 moles 15 moles 3 moles

5 moles 3/5 moles 15 moles 3 moles

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5 moles 3/5 moles 15 moles 3 moles

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  1. How many moles of CO2 are produced when 3 moles of pentane react with excess oxygen?C5H12(l) + 8O2(g)  5CO2(g) + 6H2O(l) 5 moles 3/5 moles 15 moles 3 moles

  2. How many moles of CO2 are produced when 3 moles of pentane react with excess oxygen?C5H12(l) + 8O2(g)  5CO2(g) + 6H2O(l) 5 moles 3/5 moles 15 moles 3 moles

  3. The overall equation involved in photosynthesis is 6 CO2 + 6 H2O  C6H12O6 + 6 O2.How many grams of glucose (C6H12O6, 180.1 g/mol) form when 4.40 g of CO2 react? 18.0 g 3.00 g 108 g 0.0167 g

  4. The overall equation involved in photosynthesis is 6 CO2 + 6 H2O  C6H12O6 + 6 O2.How many grams of glucose (C6H12O6, 180.1 g/mol) form when 4.40 g of CO2 react? 18.0 g 3.00 g 108 g 0.0167 g

  5. The rapid decomposition of sodium azide, NaN3, toits 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 gof NaN3? 3.88 g 1.72 g 0.138 g 2.59 g

  6. The rapid decomposition of sodium azide, NaN3, toits 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 gof NaN3? 3.88 g 1.72 g 0.138 g 2.59 g

  7. The overall equation involved in photosynthesis is 6 CO2 + 6 H2O  C6H12O6 + 6 O2.How many grams of carbon dioxide (CO2) are required to produce 18.0 g of C6H12O6? 18.0 g 3.00 g 54.0 g 26.4 g 4.40 g

  8. The overall equation involved in photosynthesis is 6 CO2 + 6 H2O  C6H12O6 + 6 O2.How many grams of carbon dioxide (CO2) are required to produce 18.0 g of C6H12O6? 18.0 g 3.00 g 54.0 g 26.4 g 4.40 g

  9. Ammonia is produced using the Haber process: 3 H2 + N2 2 NH3Calculate the mass of ammonia produced when 35.0 g of nitrogen react with 12.5 g of hydrogen. 47.5 g 42.6 g 35.0 g 63.8 g 70.5 g

  10. Ammonia is produced using the Haber process: 3 H2 + N2 2 NH3Calculate the mass of ammonia produced when 35.0 g of nitrogen react with 12.5 g of hydrogen. 47.5 g 42.6 g 35.0 g 63.8 g 70.5 g

  11. Ammonia is produced using the Haber process: 3 H2 + N2 2 NH3What percent yield of ammonia is produced from15.0 kg each of H2 and N2, if 13.7 kg of product are recovered? Assume the reaction goes to completion. 7.53 × 10–2 % 1.50 × 10–1 % 75.3% 15.0% 16.2%

  12. Ammonia is produced using the Haber process: 3 H2 + N2 2 NH3What percent yield of ammonia is produced from15.0 kg each of H2 and N2, if 13.7 kg of product are recovered? Assume the reaction goes to completion. 7.53 × 10–2 % 1.50 × 10–1 % 75.3% 15.0% 16.2%

  13. What mass of TiCl4 is needed to produce 25.0 g of Ti if the reaction proceeds with an 82% yield?TiCl4 + 2Mg  Ti + 2 MgCl2 30.5 g 121 g 99.1 g 81.2 g

  14. What mass of TiCl4 is needed to produce 25.0 g of Ti if the reaction proceeds with an 82% yield?TiCl4 + 2Mg  Ti + 2 MgCl2 30.5 g 121 g 99.1 g 81.2 g

  15. What is the molarity of an aqueous solution containing 22.5 g of sucrose (C12H22O11) in 35.5 mL of solution? • 0.0657 M • 1.85 × 10–3M • 1.85 M • 3.52 M • 0.104 M

  16. What is the molarity of an aqueous solution containing 22.5 g of sucrose (C12H22O11) in 35.5 mL of solution? • 0.0657 M • 1.85 × 10–3M • 1.85 M • 3.52 M • 0.104 M

  17. 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

  18. 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

  19. A 45.0 mL solution is 0.500 M HCl. What is the concentration after 25.0 mL of water is added to the solution? Assume volumes are additive. • 0.321 M • 0.179 M • 0.900 M • 0.278 M

  20. A 45.0 mL solution is 0.500 M HCl. What is the concentration after 25.0 mL of water is added to the solution? Assume volumes are additive. • 0.321 M • 0.179 M • 0.900 M • 0.278 M

  21. Which of the following aqueous solutions would conduct electricity? • AgNO3 • C11H22O11 (sucrose) • CH3CH2OH (ethanol) • All of the above • None of the above

  22. Which of the following aqueous solutions would conduct electricity? • AgNO3 • C11H22O11 (sucrose) • CH3CH2OH (ethanol) • All of the above • None of the above

  23. What is the maximum number of grams of PbI2 precipitated upon mixing 25.0 mL of 0.150 M KI with 15.0 mL of 0.175 M Pb(NO3)2? • 0.864 g • 1.73 g • 1.21 g • 2.07 g • None of the above

  24. What is the maximum number of grams of PbI2 precipitated upon mixing 25.0 mL of 0.150 M KI with 15.0 mL of 0.175 M Pb(NO3)2? • 0.864 g • 1.73 g • 1.21 g • 2.07 g • None of the above

  25. A 25.0 mL sample of H2SO4 is neutralized with NaOH.What is the concentration of the H2SO4 if 35.0 mL of0.150 M NaOH are required to completely neutralizethe acid? 0.210 M 0.105 M 0.150 M 0.420 M None of the above

  26. A 25.0 mL sample of H2SO4 is neutralized with NaOH.What is the concentration of the H2SO4 if 35.0 mL of0.150 M NaOH are required to completely neutralizethe acid? 0.210 M 0.105 M 0.150 M 0.420 M None of the above

  27. What mass, in grams, of sodium bicarbonate, NaHCO3, is required to neutralize 1000.0 L of 0.350 M H2SO4? • 2.94 × 104 g • 1.47 × 104 g • 5.88 × 104 g • 3.50 × 103 g • 1.75 × 103 g

  28. What mass, in grams, of sodium bicarbonate, NaHCO3, is required to neutralize 1000.0 L of 0.350 M H2SO4? • 2.94 × 104 g • 1.47 × 104 g • 5.88 × 104 g • 3.50 × 103 g • 1.75 × 103 g