Part 1: Grams, Moles and Particles

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GENERAL CHEMISTRY I CHEM 1311.002 (12681) EXAM 2 Monday, June 18, 2012 Name Banner ID Part 1: Grams, Moles and Particles 1. How many lead atoms are present in 4.216 moles of lead? Avogadro s Number is 6.022 x 10 23. a) 5.817 x 10 23 atoms b) 8.263 x 10 23 atoms c) 2.539 x 10 24 atoms d) 5.102 x 10 24 atoms e) 8.651 x 10 24 atoms 2. How many moles of magnesium are present if you have 1.560 x 10 25 magnesium atoms? Avogadro s Number is 6.022 x 10 23. a) 4.682 mol b) 6.993 mol c) 9.739 mol d) 16.82 mol e) 25.91 mol 3. How many grams of titanium are present in 0.5863 moles of titanium? The atomic weight of titanium is 47.867 g/mol. a) 4.128 g b) 8.552 g c) 17.21 g d) 28.06 g e) 40.02 g 4. How many moles are iron are present in 72.47 g of iron? The atomic weight of iron is 55.845 g/mol. a) 1.298 mol b) 2.873 mol c) 4.278 mol d) 7.316 mol e) 11.23 mol 5. How many aluminum atoms are present in 542.3 g of aluminum? Avogadro s Number is 6.022 x 10 23. The atomic weight of aluminum is 26.982 g/mol. a) 8.932 x 10 23 atoms b) 3.184 x 10 24 atoms c) 7.482 x 10 24 atoms d) 1.210 x 10 25 atoms e) 4.265 x 10 25 atoms 6. What is the mass of 4.173 x 10 24 silicon atoms? Avogadro s Number is 6.022 x 10 23. The atomic weight of silicon is 28.085 g/mol. a) 38.16 g b) 55.19 g c) 79.12 g d) 104.2 g e) 194.6 g 7. How many moles of H 2 O are present in 155.4 g of H 2 O? Atomic weights: H 1.008 g/mol O 15.999 g/mol a) 2.738 mol b) 4.572 mol c) 8.626 mol d) 12.87 mol e) 19.20 mol 8. What is the mass of 3.485 x 10 23 CO 2 molecules? Avogadro s Number is 6.022 x 10 23. Atomic weights: C 12.011 g/mol O 15.999 g/mol a) 2.733 g b) 5.101 g c) 11.22 g d) 16.31 g e) 25.47 g Part 2: Nomenclature of Binary Ionic Compounds 9. What is the formula of barium chloride? a) BaCl b) BaCl 2 c) Ba 2 Cl d) Ba 2 Cl 3 e) Ba 3 Cl 2 10. What is the formula of magnesium nitride? a) MgN b) MgN 2 c) Mg 2 N d) Mg 2 N 3 e) Mg 3 N 2 11. What is the formula of sodium sulfide? a) NaS b) NaS 2 c) Na 2 S d) Na 2 S 3 e) Na 3 S 2 12. What is the formula of aluminum phosphide? a) AlP b) AlP 2 c) Al 2 P d) Al 2 P 3 e) Al 3 P 2 13. What is the formula of aluminum oxide? a) AlO b) AlO 2 c) Al 2 O d) Al 2 O 3 e) Al 3 O 2 14. What is the formula of calcium sulfide? a) CaS b) CaS 2 c) Ca 2 S d) Ca 2 S 3 e) Ca 3 S 2 Comment [D1]: Answer Comment [D2]: Answer Comment [D3]: Answer Comment [D4]: Answer Comment [D5]: Answer Comment [D6]: Answer Comment [D7]: Answer Comment [D8]: Answer Comment [D9]: Answer Comment [D10]: Answer Comment [D11]: Answer Comment [D12]: Answer Comment [D13]: Answer Comment [D14]: Answer

15. What is the formula of sodium phosphide? a) NaP b) Na 2 P c) Na 3 P d) NaP 2 e) NaP 3 16. What is the formula of strontium bromide? a) SrBr b) Sr 2 Br c) Sr 3 Br d)srbr 2 e) SrBr 3 Part 3: Nomenclature of Ionic Compounds Containing Polyatomic Ions 17. What is the formula of sodium carbonate? a) NaCO 3 b) Na 2 CO 3 c) Na(CO 3 ) 2 d) Na 2 (CO 3 ) 3 e) Na 3 (CO 3 ) 2 18. What is the formula of potassium chlorite? a) KClO 2 b) K 2 ClO 2 c) K(ClO 2 ) 2 d) K(ClO) 2 e) K 2 (ClO) 2 Comment [D15]: Comment [D16]: Answer Comment [D17]: Answer Comment [D18]: Answer 19. What is the formula of ammonium nitrate? a) NH 4 NO 3 b) (NH 4 ) 2 NO 3 c) NH 4 (NO 3 ) 2 d) NH 4 (NO) 3 e) (NH) 4 NO 3 Comment [D19]: Answer 20. What is the formula of barium nitrite? a) BaNO 2 b) Ba 2 NO 2 c) Ba(NO 2 ) 2 d) Ba(NO) 2 e) Ba 2 (NO) 2 21. What is the formula of aluminum sulfite? a) AlSO 3 b) Al 2 SO 3 c) Al(SO 3 ) 2 d) Al 2 (SO 3 ) 3 e) Al 3 (SO 3 ) 2 22. What is the formula of calcium perchlorate? a) CaClO 4 b) Ca(ClO 4 ) 2 c) Ca 2 ClO 4 d) Ca(ClO) 4 e) Ca 2 (ClO) 4 23. What is the formula of strontium phosphate? a) SrPO 4 b) Sr(PO 4 ) 2 c) Sr 2 PO 4 d) Sr 2 (PO 4 ) 3 e) Sr 3 (PO 4 ) 2 24. What is the formula of potassium sulfate? a) KSO 4 b) K(SO 4 ) 2 c) K 2 SO 4 d) K 2 (SO 4 ) 3 e) K 3 (SO 4 ) 2 Part 4: Ions Having 2 Common Charges The Stock and -ic/-ous Systems of Nomenclature 25. What is the formula of chromium(iii) sulfide? a) CrS b) Cr 3 S c) CrS 3 d) Cr 2 S 3 e) Cr 3 S 2 26. What is the formula of iron(ii) oxide? a) FeO b) Fe 2 O c) FeO 2 d) Fe 2 O 3 e) Fe 3 O 2 27. What is the formula of lead(iv) oxide? a) PbO b) Pb 2 O c) PbO 2 d) Pb 4 O e) PbO 4 28. Copper forms the ions Cu + and Cu 2+. What is the formula of cuprous chloride? a) CuCl b) Cu 2 Cl c) CuCl 2 d) Cu 2 Cl 3 e) Cu 3 Cl 2 29. Gold forms the ions Au + and Au 3+. What is the formula of auric oxide? a) AuO b) Au 2 O c) AuO 2 d) Au 2 O 3 e) Au 3 O 2 30. Manganese forms the ions Mn 2+ and Mn 3+. Which of the following would be a correct name for MnBr 2 (in the Stock and/or -ic/-ous systems of nomenclature)? a) manganese(ii) bromide b) manganese (III) bromide c) manganous bromide d) both a and c e) both b and c 31. Tin forms the ions Sn 2+ and Sn 4+. Which of the following would be a correct name for SnF 2 (in the Stock and/or -ic/-ous systems of nomenclature)? a) tin(ii) fluoride b) tin(iv) fluoride c) stannic fluoride d) both a and c e) both b and c Comment [D20]: Answer Comment [D21]: Answer Comment [D22]: Answer Comment [D23]: Answer Comment [D24]: Answer Comment [D25]: Answer Comment [D26]: Answer Comment [D27]: Answer Comment [D28]: Answer Comment [D29]: Answer Comment [D30]: Answer Comment [D31]: Answer

32. Cobalt forms the ions Co 2+ and Co 3+. Which of the following would be a correct name for CoCl 2 (in the Stock and/or -ic/-ous systems of nomenclature)? a) cobalt(iii) chloride b) cobaltous chloride c) cobaltic chloride d) both a and b e) both a and c Part 5: Acid Nomenclature 33. What is the formula of nitrous acid? a) HNO 2 b) HNO 3 c) HNO 4 d) H 2 NO 2 e) H 2 NO 3 34, What is the name of H 2 SO 3? a) hydrosulfuric acid b) hydrosulfurous acid c) sulfuric acid d) sulfurous acid e) hyposulfuric acid 35. What is the formula of phosphoric acid? a) HPO 4 b) H 2 PO 4 c) H 3 PO 4 d) H 4 PO 4 e) H 5 PO 4 36. What is the name of HCl? a) hydrochloric acid b) hydrochlorous acid c) chloric acid d) chlorous acid e) hypochloric acid 37. What is the formula of carbonic acid? a) HCO 2 b) H 2 CO 2 c) HCO 3 d) H 2 CO 3 e) HCO 4 38. What is the name of HClO 2? a) hydrochloric acid b) hydrochlorous acid c) chloric acid d) chlorous acid e) hypochloric acid 39. What is the formula of hydrosulfuric acid? a) HS b) H 2 S c) HSO 3 d) H 2 SO 3 e) HSO 4 40. What is the name of H 2 CrO 4? a) hydrochromic acid b) hydrochromous acid c) chromic acid d) chromous acid e) hypochromic acid Part 6: Acid Salts 41. What is the formula of potassium dihydrogen phosphate? a) KH 2 PO 4 b) K(HPO 4 ) 2 c) K(H 2 PO 4 ) 2 d) K 2 HPO 4 e) K 2 H 2 PO 4 42. What is the formula of calcium bicarbonate? a) Ca(CO 3 ) 2 b) CaHCO 3 c) Ca(HCO 3 ) 2 d) CaH 2 CO 3 e) Ca(H 2 CO 3 ) 2 43. What is the formula of aluminum bisulfite? a) Al(SO 3 ) 2 b) Al(HSO 3 ) 2 c) Al(HSO 3 ) 3 d) Al(H 2 SO 3 ) 2 e) Al(H 2 SO 3 ) 3 44. What is the formula of magnesium monohydrogen phosphate? a) MgHPO 4 b) Mg 2 HPO 4 c) Mg(HPO 4 ) 2 d) MgH(PO 4 ) 2 e) MgH(PO 4 ) 3 45. What is the formula of sodium bisulfate? a) Na(SO 4 ) 2 b) NaHSO 4 c) Na 2 HSO 4 d) NaH 2 SO 4 e) Na 2 H 2 SO 4 46. What is the formula of barium hydrogen sulfide? a) BaHS b) BaHS 2 c) BaH 2 S d) Ba(HS) 2 e) Ba(H 2 S) 2 Comment [D32]: Answer Comment [D33]: Answer Comment [D34]: Answer Comment [D35]: Answer Comment [D36]: Answer Comment [D37]: Answer Comment [D38]: Answer Comment [D39]: Answer Comment [D40]: Answer Comment [D41]: Answer Comment [D42]: Answer Comment [D43]: Answer Comment [D44]: Answer Comment [D45]: Answer Comment [D46]: Answer

Part 7: Mass Percentage Calculations 47. What is the percent by mass of sodium in NaCl? Atomic weights: Na 22.990 g/mol Cl 35.453 g/mol a) 15.41% b) 24.16% c) 39.34% d) 57.22% e) 73.19% 48. What is the percent by mass of hydrogen in CH 4? Atomic weights: C 12.011 g/mol H 1.008 g/mol a) 12.83% b) 25.13% c) 41.47% d) 59.72% e) 79.20% 49. How many grams of nitrogen are present in 75.00 g of NH 3? Atomic weights: N 14.007 g/mol H 1.008 g/mol Hint: Use the chemical formula to find the mass percent of nitrogen in NH 3, then calculate that percentage of 75.00 to find the number of grams of nitrogen in 75.00 g of NH 3. a) 18.25 g b) 31.06 g c) 40.14 g d) 49.98 g e) 61.68 g 50. Mercuric oxide, HgO, is a compound of the elements mercury and oxygen. When heated, the compound decomposes. The oxygen escapes as a gas, leaving a puddle of liquid mercury. How many grams of this compound would you have to decompose in order to get 10.00 g of liquid mercury? Atomic weights: Hg 200.59 O 15.999 Hint: Use the formula HgO to calculate the mass percentage of mercury in this compound. Then determine how many grams of compound you would need to start with so that when you take that percentage of it, the result is 10.00 g. a) 10.80 g b) 15.38 g c) 24.37 g d) 39.15 g e) 55.20 g Comment [D47]: Answer Comment [D48]: Answer Comment [D49]: Answer Comment [D50]: Answer *** END OF EXAM 2 *** The remaining pages on this exam provide supplemental data to help you work the problems.

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