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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.

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Presentation on theme: "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."— Presentation transcript:

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 Answer: c

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 Answer: c

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

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

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? 3.88 g 1.72 g 0.138 g 2.59 g Answer: a

6 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? 3.88 g 1.72 g 0.138 g 2.59 g Answer: a

7 The overall equation involved in photosynthesis is
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 Answer: d

8 The overall equation involved in photosynthesis is
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 Answer: d

9 Ammonia is produced using the Haber process:
Ammonia is produced using the Haber process: 3 H2 + N2  2 NH3 Calculate 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 Answer: b

10 Ammonia is produced using the Haber process:
Ammonia is produced using the Haber process: 3 H2 + N2  2 NH3 Calculate 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 Answer: b

11 Ammonia is produced using the Haber process:
Ammonia is produced using the Haber process: 3 H2 + N2  2 NH3 What percent yield of ammonia is produced from 15.0 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% Answer: c

12 Ammonia is produced using the Haber process:
Ammonia is produced using the Haber process: 3 H2 + N2  2 NH3 What percent yield of ammonia is produced from 15.0 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% Answer: c

13 What mass of TiCl4 is needed to produce 25
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 Answer: b

14 What mass of TiCl4 is needed to produce 25
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 Answer: b

15 What is the molarity of an aqueous solution containing 22
What is the molarity of an aqueous solution containing 22.5 g of sucrose (C12H22O11) in 35.5 mL of solution? M 1.85 × 10–3 M 1.85 M 3.52 M 0.104 M Answer: c

16 What is the molarity of an aqueous solution containing 22
What is the molarity of an aqueous solution containing 22.5 g of sucrose (C12H22O11) in 35.5 mL of solution? M 1.85 × 10–3 M 1.85 M 3.52 M 0.104 M Answer: c

17 Sulfuric acid is found in some types of batteries. What volume of 3
Sulfuric acid is found in some types of batteries. What volume of 3.50 M H2SO4 is required to prepare mL of 1.25 M H2SO4? 17.5 mL 700. mL 89.3 mL 109 mL None of the above Answer: c

18 Sulfuric acid is found in some types of batteries. What volume of 3
Sulfuric acid is found in some types of batteries. What volume of 3.50 M H2SO4 is required to prepare mL of 1.25 M H2SO4? 17.5 mL 700. mL 89.3 mL 109 mL None of the above Answer: c

19 A 45.0 mL solution is 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 Answer: a

20 A 45.0 mL solution is 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 Answer: a

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

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

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

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

25 A 25. 0 mL sample of H2SO4 is neutralized with NaOH
A 25.0 mL sample of H2SO4 is neutralized with NaOH. What is the concentration of the H2SO4 if 35.0 mL of M NaOH are required to completely neutralize the acid? 0.210 M 0.105 M 0.150 M 0.420 M None of the above Answer: b

26 A 25. 0 mL sample of H2SO4 is neutralized with NaOH
A 25.0 mL sample of H2SO4 is neutralized with NaOH. What is the concentration of the H2SO4 if 35.0 mL of M NaOH are required to completely neutralize the acid? 0.210 M 0.105 M 0.150 M 0.420 M None of the above Answer: b

27 What mass, in grams, of sodium bicarbonate, NaHCO3, is required to neutralize L of M H2SO4? 2.94 × 104 g 1.47 × 104 g 5.88 × 104 g 3.50 × 103 g 1.75 × 103 g Answer: c

28 What mass, in grams, of sodium bicarbonate, NaHCO3, is required to neutralize L of M H2SO4? 2.94 × 104 g 1.47 × 104 g 5.88 × 104 g 3.50 × 103 g 1.75 × 103 g Answer: c

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