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Chemistry 107 Exam 4-6 Good Luck!. a) 18.0 g b) 3.00 g c) 108 g d) 0.0167 g 1. The overall equation involved in photosynthesis is: 6 CO 2 + 6 H 2 O 

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Presentation on theme: "Chemistry 107 Exam 4-6 Good Luck!. a) 18.0 g b) 3.00 g c) 108 g d) 0.0167 g 1. The overall equation involved in photosynthesis is: 6 CO 2 + 6 H 2 O "— Presentation transcript:

1 Chemistry 107 Exam 4-6 Good Luck!

2 a) 18.0 g b) 3.00 g c) 108 g d) g 1. The overall equation involved in photosynthesis is: 6 CO H 2 O  C 6 H 12 O O 2 How many grams of glucose (C 6 H 12 O 6 ) form when 4.40 g of CO 2 react?

3 a) 3.88 g b) 1.72 g c)0.138 g d) 2.59 g 2. The rapid decomposition of sodium azide, NaN 3, to its elements is one of the reactions used to inflate airbags: 2 NaN 3 (s)  2 Na (s) + 3 N 2 (g) How many grams of N 2 are produced from 6.00 g of NaN 3 N2N2

4 a) 7.53 x % b) 1.50 x % c) 75.3% d) 15.0% e) 16.2% 3. Ammonia is produced using the Haber process: 3 H 2 + N 2  2 NH 3 What percent yield of ammonia produced from 15.0 kg each of H 2 and N 2, if 13.7 kg of product are recovered? Assume the reaction goes to completion.

5 a) 47.5 g b) 42.6 g c) 35.0 g d) 63.8 g e) 70.5 g 4. Ammonia is produced using the Haber process: 3 H 2 + N 2  2 NH 3 Calculate the mass of ammonia produced when 35.0 g of nitrogen react with 12.5 g of hydrogen.

6 5. What mass, in grams, of sodium bicarbonate, NaHCO 3, is required to neutralize L of M H 2 SO 4 ? H 2 SO NaHCO 3  2 CO 2 + Na 2 SO H 2 O a) 2.94 x 10 4 g b) 1.47 x 10 4 g c) 5.88 x 10 4 g d) 3.50 x 10 3 g e) 1.75 x 10 3 g

7 6. Aqueous solutions of which of the following would conduct electricity? a) AgNO 3 b) C 11 H 22 O 11 (sucrose: table sugar) c) CH 3 CH 2 OH (ethanol) d) All of the above e) None of the above

8 7. Sulfuric acid is found in some types of batteries. What volume of 3.50 M H 2 SO 4 is required to prepare mL of 1.25 M H 2 SO 4 ? a) 17.5 mL b) 700. mL c) 89.3 mL d) 109 mL e) None of the above

9 N2O4N2O4 a) + 4 b) - 4 c) + 8 d) Determine the oxidation number of the Nitrogen

10 a) 18.0 g b) 3.00 g c) 54.0 g d) 26.4 g e) 4.40 g 9. The overall equation involved in photosynthesis is: 6 CO H 2 O  C 6 H 12 O O 2 How many grams of carbon dioxide (CO 2 ) are required to produce 18.0 g of C 6 H 12 O 6 ?

11 10. What is the maximum number of grams of PbI 2 precipitated upon mixing 25.0 mL of M KI with 15.0 mL of M Pb(NO 3 ) 2 ? Pb(NO 3 ) 2 + 2KI  2KNO 3 + PbI 2 a) g b) 1.73 g c) 1.21 g d) 2.07 g e) None of the above

12 11. A 25.0 mL sample of H 2 SO 4 is neutralized with NaOH. What is the concentration of the H 2 SO 4 if 35.0 mL of M NaOH are required to completely neutralize the acid? a) M b) M c) M d) M e) None of the above 2NaOH + H 2 SO 4  Na 2 SO 4 + 2H 2 O

13 12. Which of the following is a redox reaction? a) HBr (aq) + KOH (aq) → H 2 O (l) + KBr (aq) b) SO 3 (g) + H 2 O (l) → H 2 SO 4 (aq) c) HBr (aq) + Na 2 S (aq) → NaBr (aq) + H 2 S (g) d) NH 4 + (aq) + 2 O 2 (g) → H 2 O (l) + NO 3 – (aq) + 2 H + (aq) e) None of the above

14 13. What is the reducing agent in the following reaction? Zn + 2 MnO H 2 O → Zn(OH) MnO(OH) a) Zn b) MnO 2 c) H 2 O d) Zn(OH) 2 e) MnO(OH)

15 14. What is the molarity of an aqueous solution containing 22.5 g of sucrose (C 12 H 22 O 11 ) in 35.5 mL of solution? a) M b) 1.85 x M c) 1.85 M d) 3.52 M e) M

16 15. Which of the following compounds will be insoluble in water? a) Ca(OH) 2 b) Na 3 PO 4 c) CaS d) Hg 2 Cl 2 e) LiF

17 16. How many moles of helium are found in a balloon that contains 5.5 L of helium at a pressure of 1.15 atm and a temperature of 22.0 ºC? a) 3.5 b) 0.26 c) 2.6 d) 0.35 e) 3.8 Copyright © 2011 Pearson Education, Inc.

18 17. The four most common gases in the atmosphere are N 2, O 2, Ar, and CO 2. Which gas has the highest average kinetic energy at room temperature? a) N 2 b) O 2 c) Ar d) CO 2 e) All have the same average kinetic energy Copyright © 2011 Pearson Education, Inc.

19 18. The four most common gases in the atmosphere are N 2, O 2, Ar, and CO 2. Assuming all gases are in containers of equal size, temperature, and pressure, which gas has the highest density? a) All have the same density b) N 2 c) O 2 d) Ar e) CO 2 Copyright © 2011 Pearson Education, Inc.

20 19. Under what conditions would Cl 2 gas be the least ideal? a) High pressure and low temperature b) High pressure and high temperature c) Low pressure and high temperature d) Low pressure and low temperature Copyright © 2011 Pearson Education, Inc.

21 20. The volume of O 2 gas in a balloon at 1.0 atm and 305 K is 0.65 L. Calculate the volume of the gas after the temperature is lowered to 77 K while keeping the pressure and amount of O 2 constant. a) 0.16 L b) 0.65 L c) 2.8 x 10 –5 L d) 3.6 x 10 4 L e) Not enough information Copyright © 2011 Pearson Education, Inc.

22 21. Which of the following will have the greatest volume at STP? a) 5.0 g H 2 b) 5.0 g N 2 c) 5.0 g O 2 d) 5.0 g CO e) All of the above have the same volume. Copyright © 2011 Pearson Education, Inc.

23 22. A 3.50 g sample of a diatomic gas in a 1.5 L container has a pressure of 2.42 atm at 355 K. Determine the identity of the gas. a) H 2 b) N 2 c) Cl 2 d) O 2 e) F 2 Copyright © 2011 Pearson Education, Inc.

24 23. A gas phase mixture of H 2 and N 2 has a total pressure of 784 torr with an H 2 partial pressure of 124 torr. What mass of N 2 gas is present in 2.00 L of the mixture at 298 K? a) g b) g c) g d) g e) 1.99 g Copyright © 2011 Pearson Education, Inc.

25 24. What mass of water vapor is produced from the gas phase reaction of O 2 with H 2 in a 2.5 L container at 28 °C if the partial pressures of O 2 and H 2 are P O 2 = 0.98 atm and P H 2 = 1.24 atm 2 H 2 (g)+ O 2 (g)→ 2 H 2 O (g) a) 1.79 g b) 2.25 g c) 3.57 g d) 4.51 g e) 5.82 g Copyright © 2011 Pearson Education, Inc.

26 a) J b) – 649 J c) 0 J d) – 195 J e) J 25. Calculate the internal energy, ΔE, for a system that does 422 J of work and loses 227 J of energy as heat. Copyright © 2011 Pearson Education, Inc.

27 26. A 3.54 g piece of aluminum is heated to 96.2 ºC and allowed to cool to room temperature, 22.5 ºC. Calculate the heat (in kJ) associated with the cooling process. The specific heat of aluminum is J/ g · K a) b)– 236 c)+ 236 d)– e)– Copyright © 2011 Pearson Education, Inc.

28 27. The main engines of the Space Shuttle burn hydrogen to produce water. How much heat (in kJ) is associated with this process if 1.32 x 10 5 kg of liquid H 2 is burned? 2 H 2 (l ) + O 2 (l ) → 2 H 2 O (l ) ΔHº rxn = – kJ a) – b) – c) – 1.87 x d) – 3.74 x e) – 7.55 x 10 7 Copyright © 2011 Pearson Education, Inc.

29 28. A 32.5-g cube of aluminum initially at 45.8 °C is submerged into g of water at 15.4 °C. What is the final temperature of both substances at thermal equilibrium? The specific heat capacity of aluminum = J/ g °C; of water = 4.18 J/ g °C a) b) 17.3 c) –25.2 d) 39.2 e) – 39.2 Copyright © 2011 Pearson Education, Inc.

30 29. Which of the following has a negative value of ΔH? a) the combustion of gasoline b) the melting of snow c) the evaporation of ethanol d) the sublimation of CO 2 at room temperature e) All of the above have positive ΔH values. Copyright © 2011 Pearson Education, Inc.

31 30. Which of the following statements about enthalpy is false? a) The value of ΔH for a chemical reaction is the amount of heat absorbed or evolved in the reaction under conditions of constant pressure. b) An endothermic reaction has a positive ΔH and absorbs heat from the surroundings. An endothermic reaction feels cold to the touch. c) An exothermic reaction has a negative ΔH and gives off heat to the surroundings. An exothermic reaction feels warm to the touch. d) Statements (a), (b), and (c) are all false statements. e) Statements (a), (b), and (c) are all true statements. Copyright © 2011 Pearson Education, Inc.

32 31. Use Hess’s Law, determine ΔH for the target reaction below. ½ N 2 (g) + ½ O 2 (g) → NO (g) ΔH = 90.3 kJ NO (g) + ½ Cl 2 (g) → NOCl (g) ΔH = –38.6 kJ 2 NOCl (g) → N 2 (g) + O 2 (g) + Cl 2 (g) ΔH = ? a)–51.7 kJ b)51.7 kJ c)–103.4 kJ d)103.4 kJ e)142.0 kJ Copyright © 2011 Pearson Education, Inc.

33 The Answers 1. B 2. A 3. C 4. B 5. C 6. A 7. C 8. A 9. D 10. A 11. B For Fun Not on Test 12. D 13. A 14. C 15. D 16. B 17. E 18. E 19. B 20. A 21. A 22. B 23. E 24. B 25. B 26. D 27. C 28. B 29. A 30. E 31. C


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