3Mg(s) + 2FeCl 3 (s) 3MgCl 2 (s) + 2Fe(s)

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1 Exam 2 CHMY 141 F A mixture of 41.0 g of Mg and 175 g of FeCl 3 (162.2 g/mol) is allowed to react according to the reaction show below. Calculate the maximum amount of of MgCl 2 (95.21 g/mol) produced in this reaction a g b. 161 g c g d. 107 g e. 154 g 3Mg(s) + 2FeCl 3 (s) 3MgCl 2 (s) + 2Fe(s) 2. What is the percent yield for the following reaction if g of PCl 5 (208.2 g/mol) is obtained when 61.3 g of Cl 2 (70.91 g/mol) reacts with excess PCl 3? PCl 3 (g) + Cl 2 (g) PCl 5 (g) a. 195 % b % c % d % e % 3. Which of the following (dissolved in water) will give a solution with the lowest electrical conductivity? a. Sucrose, C 12 H 22 O 11 b. Sodium chloride, NaCl c. Potassium nitrate, KNO 3 d. Sulfuric acid, H 2 SO 4 e. Lithium hydroxide, LiOH 4. Sulfur dioxide reacts with chlorine to produce thionyl chloride and dichlorine oxide according to the equation shown below. If mol Cl 2 reacts with mol SO 2, how many moles of Cl 2 O are formed? a mol b mol c mol d mol e mol SO 2 (g) + 2Cl 2 (g) SOCl 2 (g) + Cl 2 O(g) 5. In the following reaction, what ions, if any, are spectator ions? a. Pb 2+ (aq), Cl (aq) b. Na + (aq), NO 3 (aq) c. Pb 2+ (aq), NO 3 (aq) d. Na + (aq), Cl (aq) e. There are no spectator ions Pb(NO 3 ) 2 (aq) + 2NaCl(aq) PbCl 2 (s) + 2NaNO 3 (aq)

2 6. Select the precipitate that forms when the following aqueous solutions are mixed. Na 2 CO 3 (aq) + BaCl 2 (aq) a. Ba 2 CO 3 b. BaCO 3 c. NaCl d. Na 2 Cl 2 e. BaO 7. What is the net ionic equation for the following reaction between sodium chloride and mercury(i) nitrate (the mercury (I) cation has the formula Hg 2 2+ ) 2NaCl(aq) + Hg 2 (NO 3 ) 2 (aq) 2NaNO 3 (aq) + Hg 2 Cl 2 (s) a. Na + (aq) + NO 3 (aq) NaNO 3 (aq) b. Hg 2 2+ (aq) + 2Cl (aq) Hg 2 Cl 2 (s) c. NaCl(aq) Na + (aq) + Cl (aq) d. Hg 2 (NO 3 ) 2 (aq) Hg 2 2+ (aq) + 2NO 3 (aq) e. 2Na + (aq) + 2Cl (aq) + Hg 2 2+ (aq) + 2NO 3 (aq) Hg 2 Cl 2 (s) + 2Na + (aq) + 2NO 3 (aq) 8. Which of the following ionic compounds is INSOLUBLE in water? a. (NH 4 ) 2 CO 3 b. AgBr c. CuSO 4 d. KI e. LiNO 3 9. Which one of the following is a strong base? a. NH 3 b. Ba(OH) 2 c. Al(OH) 3 d. CH 3 COOH e. CH 3 OH 10. Write the net ionic equation for the reaction between cesium hydroxide and hydrobromic acid: CsOH(aq) + HBr(aq) H 2 O(l) + CsBr(aq) a. CsOH(aq) Cs + (aq) + OH (aq) b. HBr (aq) + OH (aq) Br (aq) + H 2 O(l) c. H + (aq) + OH (aq) H 2 O(l) d. H + (aq) + Br (aq) + CsOH(aq) + OH (aq) Cs + (aq) + H 2 O(l) e. H + (aq) + Br (aq) + Cs + (aq) + OH (aq) Cs + (aq) + Br (aq) + H 2 O(l)

3 11. Which of the following compounds is a weak acid? a. HCl b. HClO 4 c. CH 3 CO 2 H d. HNO 3 e. HI 12. Automobile batteries use 3.0 M H 2 SO 4 as an electrolyte. How much 1.20 M NaOH will be needed to neutralize L of battery acid? H 2 SO 4 (aq) + 2NaOH(aq) 2H 2 O(l) + Na 2 SO 4 (aq) a L b L c L d L e. 1.1 L 13. The oxidation number of Cr in sodium chromite, NaCrO 2, is a. 2 b. 1 c. +1 d. +2 e Which substance in the following reaction undergoes oxidation? a. I (aq) b. I 2 (aq) c. S 4 O 6 2 (aq) d. S 2 O 3 2 (aq) e. I (aq) and S 4 O 6 2 (aq) 2S 2 O 3 2 (aq) + I 2 (aq) S 4 O 6 2 (aq) + 2I (aq) 15. What is the reducing agent in the following reaction: Cu(s) + Hg 2+ (aq) Cu 2+ (aq) + Hg(l) a. Hg 2+ (aq) b. Cu(s) c. Cu 2+ (aq) d. Hg(l) e. Hg 2+ (aq) and Cu 2+ (aq)

4 16. Calculate the molarity of ml of a solution containing g of Na 2 SO 4 ( g/mol). a M b M c M d M e M 17. How many total moles of ions are released when 0.27 mol of cobalt(ii) chloride, CoCl 2, is dissolved in water? a mol b mol c mol d mol e mol 18. A normal saline solution used for intravenous infusion is commonly M NaCl. Calculate the mass of NaCl needed to prepare ml of a normal saline solution. a. 41.3g b g c g d g e g 19. How many ml of concentrated nitric acid (HNO 3, 16.0 M) should be diluted with water in order to make 2.00 L of 2.00 M solution? a ml b ml c. 125 ml d ml e ml 20. How many milliliters of 1.58 M HCl are needed to react completely with 23.2 g of NaHCO 3 (84.02 g/mol), according to the following reaction: HCl(aq) + NaHCO 3 (aq) NaCl(aq) + H 2 O(l) + CO 2 (g) a. 638 ml b. 572 ml c. 536 ml d. 276 ml e. 175 ml

5 21. Which one of the following statements is INCORRECT? a. Energy is neither created nor destroyed in chemical reactions. b. Kinetic energy is the energy associated with motion. c. Endothermic processes absorb heat from the surrounding into the system. d. Potential energy is the energy of position. e. Potential energy and kinetic energy are not interconvertible. 22. A Snickers candy bar contains 280 Calories, of which the fat content accounts for 120 Calories. What is the energy of the fat content, in kj? (4.184 J = 1 cal) a kj b. 29 kj c. 5.0 x10 2 kj d kj e. 5.0 x10 5 kj 23. Which of the following is not a state function? a. internal energy b. volume c. work d. pressure e. enthalpy 24. Calculate the heat change (q) in kj when 28.6 g of water is heated from 22.0 C to 78.3 C. (Specific heat capacity of water = J/g C ). a kj b kj c kj d kj e x10 3 kj 25. A system absorbs 575 J of heat and does 425 J of work on the surroundings. Calculate the change in the internal energy, U. a. 150 J b J c J d J e J

6 26. The Starship Enterprise is caught in a time warp and Spock is forced to use the primitive techniques of the 20th century to determine the specific heat capacity of an unknown mineral. A 307 g sample of the mineral was heated to 98.7 C and placed into 76.2 g of water initially at 23.6 C. The final temperature of the water & mineral sample was 32.4 C. What is the specific heat capacity of the mineral? (Sp. heat capacity of water = J/g C ) a J/g C b J/g C c J/g C d J/g C e J/g C 27. Which one of the following equations represents the standard enthalpy of formation reaction for CH 3 OH(l)? a. C (g) + 2 H 2 (g) + 1/2 O 2 (g) CH 3 OH (l) b. C (g) + 4H (g) + O (g) CH 3 OH (l) c. C (graphite) + 4 H (g) + O(g) CH 3 OH (l) d. C (diamond) + 2 H 2 (g) + O(g) CH 3 OH (l) e. C (graphite) + 2 H 2 (g) + 1/2 O 2 (g) CH 3 OH (l) 28. Using the standard reaction enthalpies provided below and Hess s law, determine the ΔH value for the reaction : Fe 2 O 3 (s) + CO(g) 2FeO(s) + CO 2 (g) Fe 2 O 3 (s) + 3CO(g) 2Fe(s) + 3CO 2 (g) FeO(s) + CO(g) Fe(s) + CO 2 (g) H = 26.8 kj H = 16.5 kj a kj b kj c, 6.2 kj d kj e kj

7 29. Galena, PbS(s), is the ore from which elemental lead is extracted. In the first step of the extraction process shown below, galena is heated in air to form lead(ii) oxide, PbO. What mass of PbS (s) will result in the release of 975 kj of heat? 2PbS(s) + 3O 2 (g) 2PbO(s) + 2SO 2 (g) H = kj/mol rxn a. 203 g b. 282 g c. 406 g d. 478 g e. 564 g 30. Calculate H for the following reaction using the standard molar enthalpy of formation data provided. SiO 2 (s) + 4HCl(g) SiCl 4 (g) + 2H 2 O(g) H f: kj/mol a kj b kj c kj d kj e kj

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