Exam 1 Worksheet Chemistry 102

Transcription

1 Exam 1 Worksheet Chemistry 102 Chapter 1 Introduction 1. Convert: a. 650 nm to inches b. 650 km to miles c. 345 mg to lb d. 145 lb to μg e km to μm f mg to Mg g ml to kl h. 455 nm to km i yards to cm j gallons to ml k. 5.5 cups to μl l. 56 ºF to ºC m. 56 ºF to K n. 56 ºC to K o. 56 K to ºC p. 56 K to ºF 2. Give the density for the substances: a. A 3.45 μg cube of silver with an edge length of ft. b. A 5.60 kg cube of gold with an edge length of μm. c. An irregular sample of lead with a mass of lb that when placed in ml of water records a final reading of ml. d moles of nitrogen gas in 10.0 L. 3. Determine the mass of a gallon of water in lb. (use the density of water = 1.0 g / ml) Chapter 2 Atoms, Molecules and Ions 4. Give the nuclear symbol for the following: a. A species with 18 electrons and a charge of 4+ b. Two possible isotopes for zinc c. The 1% abundant isotope for carbon d. A species with 48 electrons and a charge of 2+ e. A species with 36 electrons and a charge of 1 f. Two isotopes of chlorine (chlorine 36 does not exist) 5. Give all of the information from the following nuclear symbols: 7 a. 3 Li+ 1

2 b. c. d. e. 40 Ar Ag+ 90 Zr I 6. Determine the relative abundance of the only two isotopes of carbon: carbon 12 with a mass of a.m.u. and carbon 13 with a mass of a.m.u. 7. Determine the mass of neon 22 when neon has two isotopes and neon 20 has a mass of a.m.u. and a relative abundance of 90.51%. 8. Give the name of the following combinations or formulas a. LiOH b. MgCO 3 c. Zn(NO 3 ) 2 d. AlPO 3 e. CO 2 f. CO g. N 2 O h. NCl 3 i. ICl 7 j. K 2 O k. Calcium and fluorine l. Aluminum and oxygen m. C 2 H 3 O 2 and silver n. Cadmium and nitrate 9. Give the formula for the following combinations or names a. Silicon dioxide b. Copper(I) oxide c. Calcium phosphate d. Chromium(III) sulfite e. Nitrite and magnesium f. Nitrogen monoxide g. Sodium nitride h. Carbon tetrachloride i. Cadmium sulfide j. Carbon disulfide k. Zinc and hydroxide l. Calcium and fluorine m. Aluminum and oxygen n. C 2 H 3 O 2 and Fe 3+ 2

3 Chapter 3 Stoichiometry 10. Give the number of molecules, the number of oxygen atoms, and the total number of atoms in the following. a moles of carbon dioxide b g of carbon dioxide c g of nitrogen monoxide d g of oxygen e g of diphosphorus pentoxide f mol of diphosphorus pentoxide 11. Give the percent composition of oxygen in the following samples. a g of potassium oxide b. Lithium hydroxide c. Barium hydroxide d g of aluminum sulfite e. 3.4 g of water f. Ammonium phosphite g g of zinc carbonate h. Gold(III) sulfate i. Magnesium nitrite 12. Give the mass of oxygen in the following samples. a g of potassium oxide b g of lithium hydroxide c g of barium hydroxide d g of aluminum sulfite e. 3.4 g of water f g of ammonium phosphite g g of zinc carbonate h g of gold(iii) sulfate i g magnesium nitrite 13. Determine the empirical and molecular formulas for the following g samples: a. Molar mass = g mol % carbon and the remainder is hydrogen b. Molar mass = g mol g oxygen, g hydrogen, and the remainder is carbon c. Molar mass = g mol % carbon and the remainder is hydrogen d. Molar mass = g mol % carbon, g nitrogen, and the remainder is hydrogen e. Molar mass = g mol g hydrogen, % nitrogen, and the remainder is carbon 3

4 f. Molar mass = g mol % carbon, g hydrogen, and the remainder is chlorine 14. Stoichiometry Using the following balanced chemical equation, determine the following 2Al NO aq + 3Na CO aq 6NaNO aq + Al CO s ( ) ( ) ( ) ( ) ( )() a. The mass of sodium carbonate needed to make 34.5 g of aluminum carbonate. b. The mass of sodium nitrate produced from g of aluminum nitrate. c. The mass of aluminum nitrate needed to produce 4.50 g of aluminum carbonate. d. The mass of aluminum carbonate produced from 4.50 g of aluminum nitrate. e. The total number of atoms reacted when 3.45 g of aluminum carbonate is f. The total number of atoms reacted when 3.45 g of sodium nitrate is g. The total number of atoms produced when 3.45 g of sodium carbonate is reacted. h. The total number of atoms produced when 3.45 g of aluminum nitrate is reacted. 15. Use the following balanced chemical reaction to answer the following: Fe2O3( s) + 3CO( g) 2Fe ( l) + 3CO2( g) a. Determine the mass of iron produced when 5.60 kg of iron(iii) oxide are reacted. b. Determine the mass of carbon monoxide are reacted when 10.6 kg of carbon dioxide are c. Determine the mass of iron(iii) oxide reacted when L of carbon dioxide is produced (density = 1.96 g L 1 ) d. Determine the volume of carbon dioxide produced when 560 kg of iron is also e. Determine the volume of carbon dioxide produced when 560 kg of iron(iii) oxide is reacted. f. Determine the volume of carbon monoxide reacted when 1000 L of carbon dioxide produced (density of CO = 1.25 g L 1 ) g. Determine the volume of carbon monoxide reacted when 14.5 kg of iron is h. Determine the volume of carbon monoxide reacted when 14.5 kg of iron(iii) oxide is also reacted. i. Determine the number of carbon dioxide molecules produced when 32.5 μg of iron(iii) oxide is reacted. j. Determine the number of carbon monoxide molecules reacted when 3.25 μg of iron is k. Determine the number of carbon dioxide molecules produced when 3.25 μg of iron is also l. Determine the number of carbon monoxide molecules reacted when 32.5 μg of iron(iii) oxide is also reacted. 4

5 16. Limiting reactant For the following balanced chemical reaction, determine the following: 2 NH PO aq + 3Cu C H O aq Cu PO s + 6NH C H O aq ( ) ( ) ( ) ( ) ( ) ( ) ( ) a. Determine the limiting reactant and theoretical yield (in mass of product) for the following combinations. i g each of both reactants. ii g of ammonium phosphate and 35.0 g of copper(ii) acetate. iii g of ammonium phosphate and 45.0 g of copper(ii) acetate. iv g of ammonium phosphate and g of copper(ii) acetate. v g of ammonium phosphate and g of copper(ii) acetate. vi ml each of a 1.35 M solution of both reactants. vii ml of a 1.67 M of ammonium phosphate and 13.5 ml of a 5.67 M solution of copper(ii) acetate. viii ml of a M solution of copper(ii) acetate and ml of a 1.45 M solution of ammonium phosphate. ix. 125 ml of a M solution of ammonium phosphate and 56.0 g of copper (II) acetate. x. 156 ml of a M solution of copper(ii) acetate and g of ammonium phosphate. b. For each of the calculations in part (a), determine the percent yield of the reactant if g of solid product is obtained. c. For each of the percent yields determined in part (b), comment on the validity of the experiment. d. Using only valid percent yields from part (b), determine the mass of solid product expected if 1235 g of each reactant is used. 5