# FINAL EXAM CHEM 1310 FS11 VERSION GREEN

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1 FINAL EXAM CHEM 1310 FS11 VERSION GREEN Name: 1. How many liters of chlorine gas at 25 C and atm can be produced by the reaction of 12.0 g of MnO 2? MnO 2 (s) + 4HCl(aq) MnCl 2 (aq) + 2H 2 O(l) + Cl 2 (g) A) 3.55 L B) 3.09 L C) L D) L E) L 2. A 6.0-ft person weighs 168 lb. What is this person's height in meters and weight in kilograms? (1 lb = g; 1 m = 3.28 ft.) A) 5.4 m, 76.2 kg B) 1.8 m, 76.2 kg C) 2.3 m, 43.2 kg D) 1.8 m, 7620 kg 3. The speed of sound in air at room temperature is about 343 m/s. What is this speed in miles per hour? (1 mi = 1609 m.) A) 12.8 mph B) 343 mph C) 767 mph D) mph 4. The oxidation number of Fe in K 3 Fe(CN) 6 is A) 3 B) +3 C) +2 D) 4 E) What is 25.4 mg when converted to kilograms? A) 2.54 kg B) kg C) kg D) 2540 kg 6. What is the formula for copper (II) cyanide? A) Cu(CN) 2 B) Cu 2 CN C) CuNCO D) CuCN Version 1 Page 1

2 7. What is the molar mass of acetaminophen, C 8 H 9 NO 2? A) 125 g/mol B) 162 g/mol C) 76 g/mol D) 43 g/mol E) 151 g/mol 8. Calculate the mass of iron(ii) sulfide formed when g of Fe reacts with g of S. A) 9.17 g B) 5.27 g C) g D) g E) g 9. Aluminum is a lightweight metal (density = 2.70 g/cm 3 ) used in aircraft construction, high-voltage transmission lines, beverage cans, and foils. What is its density in kg/m 3? A) kg/m 3 B) kg/m 3 C) kg/m 3 D) kg/m How many atoms are in 5.54 g of F 2? A) atoms B) atoms C) atoms D) atoms E) atoms 11. A sample of air occupies 3.8 L when the pressure is 1.2 atm. What volume does it occupy at 6.6 atm? (The temperature is kept constant.) A) 0.69 L B) 20.9 L C) 0.58 L D) 30.1 L 12. Under what set of conditions would a gas be expected to behave most ideally? A) High temperature and high pressure B) Low temperature and low pressure. C) High temperature and low pressure D) Low temperature and high pressure Version 1 Page 2

3 13. Calculate the density, in g/l, of SF 6 gas at 27 C and atm pressure. A) 3.38 kg/l B) 22.4 g/l C) g/l D) 2.96 g/l E) 32.9 g/l 14. Based on the solubility rules, which one of the following should be soluble in water? A) K 2 SO 4 B) AgCl C) BaSO 4 D) PbSO 4 E) CaSO When potassium cyanide (KCN) reacts with acids, a deadly poisonous gas, hydrogen cyanide (HCN), is given off. Here is the equation: KCN(aq) + HCl(aq) KCl(aq) + HCN(g) If a sample of g of KCN is treated with an excess of HCl, calculate the amount of HCN formed, in grams. A) g B) g C) g D) g 16. Based on the solubility rules, which one of the following compounds should be insoluble in water? A) FeCl 2 B) AgBr C) ZnCl 2 D) NaCl E) MgBr The correct name for KHCO 3 is A) potassium hydrogen carbonate. B) potassium carbonate. C) calcium bicarbonate. D) calcium carbonate. E) calcium hydrogen carbon trioxide. Version 1 Page 3

4 18. The mineral hausmannite is a compound of manganese-55 and oxygen-16. If 72% of the mass of hausmannite is due to manganese, what is the empirical formula of hausmannite? A) Mn 3 O 4 B) Mn 4 O 3 C) MnO 3 D) MnO E) Mn 3 O 19. The temperature of an ideal gas in a 5.00 L container originally at 1 atm pressure and 25 C is lowered to 220. K. Calculate the new pressure of the gas. A) 8.8 atm B) atm C) 1.35 atm D) 1.0 atm E) atm 20. What is the formula for the binary compound formed by potassium and nitrogen? A) K 2 N B) NK 2 C) NK 3 D) KN E) K 3 N 21. Calculate the sodium ion concentration in a solution formed by diluting ml of a M sodium phosphate solution to a final volume of ml. A) M B) 11.9 M C) 3.96 M D) M E) M 22. How many grams of sulfur are there in 6.0 g of Fe 2 (SO 4 ) 3? A) 6.00 g B) 0.92 g C) 0.48 g D) 1.44 g E) 2.40 g Version 1 Page 4

5 23. What mass of K 2 CO 3 is needed to prepare 200. ml of a solution having a potassium ion concentration of M? A) 1.49 g B) 2.07 g C) 4.15 g D) 13.8 g E) 10.4 g 24. The density of mercury is 13.6 g/cm 3. How may liters does 325 g of Hg occupy? A) 4.42 x 10 6 L B) 4.42 x 10 3 L C) 2.39 x 10 4 L D) x 10 0 L E) 2.39 x 10 2 L 25. Why is magnesium chloride (MgCl 2 ) not called magnesium(ii) chloride? A) Only iron and copper use the Roman numeral convention. B) The magnesium in MgCl 2 does not have a charge of 2+. C) Magnesium (II) is the only common ion of magnesium. D) Magnesium chloride is not ionic. 26. What is the chemical formula of the salt produced by the neutralization of nitric acid with calcium hydroxide? A) Ca 3 (NO 3 ) 2 B) Ca 2 NO 3 C) Ca(NO 3 ) 2 D) CaNO 3 E) Ca 2 (NO 3 ) How many moles of HCl are represented by HCl molecules? A) 36.5 mol B) mol C) mol D) mol E) mol 28. Express 7,500 nm as picometers. A) 75.0 pm B) 750 pm C) pm D) pm E) 7.50 pm Version 1 Page 5

6 29. Consider the reaction MnO 2 + 4HCl MnCl 2 + Cl 2 + 2H 2 O If 0.86 mole of MnO 2 and 48.2 g of HCl react, how many grams of Cl 2 will be produced? A) 23.4 g B) 42.3 g C) 93.6 g D) 63.4 g 30. When 20.0 ml of a M (NH 4 ) 2 S solution is added to ml of a solution of Cu(NO 3 ) 2, a CuS precipitate forms. The precipitate is then filtered from the solution, dried, and weighed. If the recovered CuS is found to have a mass of g, what was the concentration of copper ions in the original Cu(NO 3 ) 2 solution? A) M B) M C) M D) M E) M 31. A slow jogger runs a mile in 13 min. Calculate the speed in km/h. (1 mi = 1609 m) A) 0.74 km/hr B) 2.9 km/hr C) 7.4 km/hr D) 3.5 km/hr 32. The stock system name for CrSO 3 is: A) chromium(ii) sulfate B) chromium(iii) sulfite C) chromium sulfur oxide D) chromium sulfide E) chromium(ii) sulfite 33. At 741 torr and 44 C, 7.10 g of a gas occupy a volume of 5.40 L. What is the molar mass of the gas? A) 46.0 g/mol B) 35.0 g/mol C) 20.3 g/mol D) 4.85 g/mol Version 1 Page 6

7 34. Determine the molar mass of Freon-11 gas if a sample weighing g occupies 100. cm 3 at 95 C, and 1,000. mmhg. A) 384 g/mol B) 70.9 g/mol C) 0.19 g/mol D) 35.3 g/mol E) 137 g/mol 35. Which of the following compounds is named lithium carbonate? A) LiHCO 3 B) LiCO C) Li 2 CO 3 D) Na 2 CO 3 Version 1 Page 7

8 Answer Key 1. A 2. B 3. C 4. B 5. C 6. A 7. E 8. C 9. B 10. C 11. A 12. C 13. D 14. A 15. B 16. B 17. A 18. A 19. E 20. E 21. A 22. D 23. B 24. E 25. C 26. C 27. E 28. C 29. A 30. E 31. C 32. E 33. B 34. E 35. C Version 1 Page 8

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