2. 1.What information would you need to calculate the average atomic mass of an element? A.The number of neutrons in the element. B.The atomic number of the element. C.The mass and abundance of each isotope of the element. * D.The position in the periodic table of the element. 2.The atomic masses of Cl (75.53 %) and Cl (24.47 %) are 34.968 amu and 36.956 amu, respectively. Calculate the average atomic mass of chlorine. A.35.96 amu B.35.45 amu * C.36.47 amu D.71.92 amu 3.How many atoms are there in 5.10 moles of sulfur ( 16 S=32 amu)? A.3.07 x 10 24 * B.9.59 x 10 22 C.6.02 x 10 23 D.9.82 x 10 25 2

3. Percent abundance (%)Mass of isotope (amu) 92.23 4.67 3.10 27.977 28.977 29.974 4. An element X, has three stable isotopes: Calculate its average atomic mass A.29.3 amu B.28.1 amu * C.27.0 amu D.30.2 amu 5.Determine the mass percent of Nitrogen in Fe 4 [Fe(CN) 6 ] 3 : A.58.7 % N B.0.2 % N C.58 % N D.29.3 % N *

4. 6. Which of the following organic compounds has the highest molecular weight? A.C 3 H 8 B.C 6 H 10 O 2 * C.C 2 H 10 O 3 D.C 2 H 6 O 7. this equation can be read as: A.2 atoms of magnesium combine with 1 molecule of oxygen to form 2 molecules of magnesium oxide. B.2 moles of magnesium combine with 1 mole of oxygen to form 2 moles of magnesium oxide. C.Both A and B are true. * D.None of the above.

5. 8.Iodine has two isotopes 126 I and 127 I, with the equal abundance. Calculate the average atomic mass of Iodine ( 53 I). A.126.5 amu * B.35.45 amu C.1.265 amu D.71.92 amu 9.The atomic masses of 6 Li and 7 Li are 6.0151 amu and 7.0160 amu, respectively. Calculate the natural abanduce of these two isotopes. The average atomic mass of Lithium (Li=6.941 amu). A. 6 Li= 7.49%, 7 Li= 92.51% * B. 7 Li= 7.49%, 6 Li= 92.51% C. 6 Li= 8.49%, 7 Li= 95.51% D. 7 Li= 7.22%, 6 Li= 82.51% 10.How many atoms are present in 3.14 g of copper (Cu)? A.2.98 x 10 22 * B.1.92 x 10 23 C.1.89 x 10 24 D.6.02 x 10 23

6. 12.What is the empirical formula of a compound that contain 50% Sulfur and 50% Oxygen. A.S 2 O B.SO 2 * C.SO D.S 2 O 3 13. What is the molecular formula of a compound that has a molar mass 213 g/mol, and an empirical formula C 2 HNO 2. A.C 2 HNO 2 B.C 4 H 2 N 2 O 4 C.C 6 H 3 N 3 O 6 * D.C 10 H 4 N 4 O 6 11. the correct coefficients for the balanced equation below are: A.2,3,1,3 * B.2,1,2,3 C.1,1,2,3 D.2,1,1,1

7. 14.Calculate the molar mass of Li 2 CO 3. A.73.89 g * B.66.95 g C.41.89 g D.96.02 g 15.How many molecules of ethane (C 2 H 6 ) are present in 0.334 g of C 2 H 6 ? A.2.01 x 10 23 B.6.69 x 10 21 * C.4.96 x 10 22 D.8.89 x 10 20 7 16.All of the substances listed below are fertilizers that contribute nitrogen to the soil. Which of these is the richest source of nitrogen on a mass percentage basis? A.Urea, (NH 2 ) 2 CO B.Ammonium nitrate, NH 4 NO 3 C.Guanidine, HNC(NH 2 ) 2 D.Ammonia, NH 3 *

8. 17. the mass of one molecule of oxygen gas is about : 18.What is the mass in grams of a single atom of As? A) * 1.244 x 10 -22 g B)2.217 x 10 -26 g C)8.039 x 10 21 g D)4.510 x10 25 g

9. 19.Allicin is the compound responsible for the characteristic smell of garlic. An analysis of the compound gives the following percent composition by mass: C: 44.4 percent; H: 6.21 percent; S: 39.5 percent; O: 9.86 percent. What is its molecular formula given that its molar mass is about 162 g? A.C 12 H 20 S 4 O 2 B.C 7 H 14 SO C.C 6 H 10 S 2 O * D.C 5 H 12 S 2 O 2 20.The formula for rust can be represented by Fe 2 O 3. How many moles of Fe are present in 24.6 g of the compound? A.2.13 mol B.0.456 mol C.0.154 mol D.0.308 mol * 9 21. What is the mass, in grams, of one copper atom? A. 1.055  10 -22 g * B. 63.55 g C. 1 amu D. 1.66  10 -24 g E. 9.476  10 21 g

10. 22.How many grams of sulfur (S) are needed to react completely with 246 g of mercury (Hg) to form HgS? A.39.3 g * B.24.6 g C.9.66 × 10 3 g D.201 g 23.Tin(II) fluoride (SnF 2 ) is often added to toothpaste as an ingredient to prevent tooth decay. What is the mass of F in grams in 24.6 g of the compound? A.18.6 g B.24.3 g C.5.97 g * D.75.7 g 24.What is the empirical formula of the compound with the following composition? 2.1 percent H, 65.3 percent O, 32.6 percent S. A.H 2 SO 4 * B.H 2 SO 3 C.H2S2O3H2S2O3 D.HSO 3 10

11. 25. Determine the number of moles of aluminum in 96.7 g of Al. A. 0.279 mol B.3.58 mol* C.7.43 mol D.4.21 mol E.6.02  10 23 mol 26. Which of the following samples contains the greatest number of atoms? A. 100 g of Pb B.2.0 mole of Ar * C.0.1 mole of Fe D.5 g of He E.20 million O 2 molecules 27. Formaldehyde has the formula CH 2 O. How many molecules are there in 0.11 g of formaldehyde? A. 6.1  10 -27 molecule B.3.7  10 -3 molecule C.4  10 21 molecule D.2.2  10 21 molecule * E.6.6  10 22 molecule

12. 28. How many sulfur atoms are present in 25.6 g of Al 2 (S 2 O 3 ) 3 ? A. 0.393 B. 6 C. 3.95  10 22 D. 7.90  10 22 E. 2.37  10 23 * 29. What is the coefficient of H 2 O when the following equation is properly balanced with the smallest set of whole numbers? ___ Al 4 C 3 + ___ H 2 O  ___ Al(OH) 3 + ___ CH 4 A. 3 B. 4 C. 6 D. 12 * E. 24 30. Which of the following equations is balanced? A.2C + O 2 CO B.2CO + O 2 2CO 2 * C.H 2 + Br 2 HBr D.2K + H 2 O 2KOH + H 2

13. 31. When 22.0 g NaCl and 21.0 g H 2 SO 4 are mixed and react according to the equation below, which is the limiting reagent? 2NaCl + H 2 SO 4  Na 2 SO 4 + 2HCl A. NaCl * B. H 2 SO 4 C. Na 2 SO 4 D. HCl E. No reagent is limiting. 32. Hydrochloric acid can be prepared by the following reaction: 2NaCl(s) + H 2 SO 4 (aq)  2HCl(g) + Na 2 SO 4 (s) How many grams of HCl can be prepared from 2.00 mol H 2 SO 4 and 150 g NaCl? A.7.30 g B.93.5 g * C.146 g D.150 g E.196 g

14. 33. What is the theoretical yield of chromium that can be produced by the reaction of 40.0 g of Cr 2 O 3 with 8.00 g of aluminum according to the chemical equation below? 2Al + Cr 2 O 3  Al 2 O 3 + 2Cr A. 7.7 g B. 15.4 g * C. 27.3 g D. 30.8 g E. 49.9 g 34. Hydrogen fluoride is used in the manufacture of Freons (which destroy ozone in the stratosphere) and in the production of aluminum metal. It is prepared by the reaction CaF 2 + H 2 SO 4 CaSO 4 + 2HF In one process 6.00 kg of CaF 2 are treated with an excess of H 2 SO 4 and yield 2.86 kg of HF. Calculate the percent yield of HF. A.93.0 % * B.95.3 % C.47.6 % D.62.5 %

15. 35.Consider the combustion of carbon monoxide (CO) in oxygen gas: 2CO(g) + O 2 (g) 2CO 2 (g) Starting with 3.60 moles of CO, calculate the number of moles of CO 2 produced if there is enough oxygen gas to react with all of the CO. A.7.20 mol B.44.0 mol C.3.60 mol * D.1.80 mol 36.Nitrous oxide (N 2 O) is also called “laughing gas.” It can be prepared by the thermal decomposition of ammonium nitrate (NH 4 NO 3 ). The other product is H 2 O. The balanced equation for this reaction is: NH 4 NO 3 N 2 O + 2H 2 O How many grams of N 2 O are formed if 0.46 mole of NH 4 NO 3 is used in the reaction? A.2.0 g B.3.7 10 1 g C.2.0 10 1 g * D.4.6 10 -1 g

16. 37.Nitric oxide (NO) reacts with oxygen gas to form nitrogen dioxide (NO 2 ), a dark-brown gas: 2NO(g) + O 2 (g) 2NO 2 (g) In one experiment 0.886 mole of NO is mixed with 0.503 mole of O 2. Calculate the number of moles of NO 2 produced (note: first determine which is the limiting reagent). A)0.886 mol * B)0.503 mol C)1.01 mol D)1.77 mol 16 38.The fertilizer ammonium sulfate [(NH 4 ) 2 SO 4 ] is prepared by the reaction between ammonia (NH 3 ) and sulfuric acid: 2NH 3 (g) + H 2 SO 4 (aq) (NH 4 ) 2 SO 4 (aq) How many kilograms of NH 3 are needed to produce 1.00 x 10 5 kg of (NH 4 ) 2 SO 4 ? A)1.70 10 4 kg B)3.22 10 3 kg C)2.58 10 4 kg * D)7.42 10 4 kg

17. 17 41. Calculate the percent of nitrogen in Mg(NO 3 ) 2 A. 18.89% * B. 9.44% C. 17.10% D. 16% 40. How many grams of NO 2 are there in 1.55 mol of NO 2 ? A. 71.32 g * B. 199 g C. 80.01 g D. 200 g 39. What is the number of oxygen atoms in 3 mol of SO 2 ? A. 5X10 24 B. 3.6X10 24 C. 2X10 23 D. 6 42. Reaction of 1.00 mole CH 4 with excess Cl 2 yields 96.8 g CCl 4. What is the percent yield of CCl 4 ? (Atomic weights: C = 12.01, Cl = 35.45). CH 4 + 4 Cl 2 CCl 4 + 4 HCl A. 64.3% B. 57.3% C. 65.9% D. 62.9% *

18. 1. What mass of K 2 CO 3 is needed to prepare 200. mL of a solution having a potassium ion concentration of 0.150 M? A.4.15 g B.10.4 g C.13.8 g D.2.07 g 2. A 50.0 mL sample of 0.436 M NH 4 NO 3 is diluted with water to a total volume of 250.0 mL. What is the ammonium nitrate concentration in the resulting solution? A.21.8 M B.0.459 M C.2.18  10 -2 M D.8.72  10 -2 M 3. A 3.682 g sample of KClO 3 is dissolved in enough water to give 375. mL of solution. What is the chlorate ion concentration in this solution? A. 3.00  10 -2 M B. 4.41  10 -2 M C. 0.118 M D. 1.65  10 -2 M E. 8.01  10 -2 M

19. 4. 25.0 mL of a 0.2450 M NH 4 Cl solution is added to 55.5 mL of 0.1655 M FeCl 3. What is the concentration of chloride ion in the final solution? A.0.607 M B.0.418 M * C.1.35 M D.0.190 M E.0.276 M 5. How many milliliters would you need to prepare 60.0 mL of 0.200M HNO 3 from a stock solution of 4.00M HNO 3 ? A. 3 mL * B. 240 mL C. 24 mL D. 1000 mL 6. What volume, in mL, of a 3.89 x 10 -2 M solution is required to provide 2.12 g of KBr? (Atomic weights: K = 39.10, Br = 79.90). A. 520 mL B. 458 mL * C. 389 mL D. 325 mL