2. The accepted density for copper is 8.96 g/ml. Calculate the percent error for a measurement of 8.86 g/ml.

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1 Chem nd Semester Exam Review Worksheet (answers and units are at the end of this worksheet, cross them off as you write down the answers to each question.) 1. Round to the correct number of significant figures: a. (8.54 x 10-3 ) (3.41 x 10-4 ) = b = c. 45 x 72 x 132 = d / 4784 = 2. The accepted density for copper is 8.96 g/ml. Calculate the percent error for a measurement of 8.86 g/ml. 3. How many electrons, protons, and neutrons are in the following? a. Ti-48 b. 132 Cs Silver has two isotopes: Ag-107 has a mass of amu (52.00%) and Ag-109 has a mass of amu (48.00%). What is the atomic mass of silver? 5. Given the electron configuration, name the element: a. 1s 2 2s 2 2p 3 b. [Ne]3s 2 3p 4 c. Write the electron configuration of magnesium (not in answers). 6. a. Which of the following has the largest atomic radius: N, Sb, As? b. Which of the following has the smallest atomic radius: Na, Mg, K, Ca? c. Which of the following has the smallest ionic radius: S, Cl, Se, Br? d. It can be predicted that silicon will experience a large jump in ionization energy after its ionization. 7. Write the formula for the ionic compound composed of: a. cesium and nitride b. aluminum and bromide 1

2 c. calcium and carbonate d. sodium and sulfite e. ammonium and phosphate 8. Name the following: a. As 2O 3 b. N 2F 4 c. H 2Se d. HClO 3 9. What is the molecular geometry of the following: a. SCl 2 b. AlCl 3 c. PH 3 d. CCl 4 e. SF Polar or nonpolar: a. NCl 3 b. BF 3 c. CS 2 d. ClF 11. Predict the products (write NR if no reaction): a. Al + S b. C 2H 6 + O 2 c. NaN 3 d. Ni + MgCl 2 e. Ca + CuBr 2 f. F 2 + FeI 2 g. Br 2 + CoCl a. How many representative particles are there in mol silver? 2

3 b. How many moles are there in 1.56 x formula units of sodium hydroxide? c. How many molecules are there in mol As 2O 3? d. How many moles are there in 1.25 x molecules CO 2? e. How many grams are there in 4.22 x atoms of U? f. How many moles of oxygen atoms are contained in 2.50 mol KMnO 4? g. How many moles of Al ions are in 45.0 g aluminum oxide? h. How many formula units are present in g lead(ii) chloride? i. Calculate the mass of 3.62 x molecules of C 6H 12O Express the composition of Al 2(SO 4) 3 as the mass percent of its elements (percent composition). 14. Monosodium glutamate (MSG) is sometimes added to food to enhance flavor. Analysis determined this compound to be 35.5% C, 4.77% H, 8.29% N, 13.6% Na, and 37.9% O. What is the empirical formula for MSG? 3

4 15. Glycerol is a thick, sweet liquid obtained as a byproduct of the manufacture of soap. Its percent composition is 39.12% carbon, 8.75% hydrogen, and 52.12% oxygen. The molar mass is g/mol. What is the molecular formula for glycerol? 16. Carbon dioxide is released into the atmosphere through the combustion of octane (C 8H 18) in gasoline. Write the balanced chemical equation for the combustion of octane and calculate the mass of octane needed to release 5.00 mol CO Chloroform (CHCl 3), and important solvent, is produced by a reaction between methane and chlorine. CH 4(g) + 3Cl 2(g) CHCl 3(g) + 3HCl(g) How many g CH 4 is needed to produce 50.0 g CHCl 3? 18. An alkaline battery produces electrical energy according to this equation. Zn(s) + 2MnO 2(s) + H2O(l) Zn(OH) 2(s) + Mn 2O 3(s) a) Determine the limiting reactant if 25.0 g Zn and 30.0 g MnO 2 are used. b) Determine the mass of Zn(OH) 2 produced. 4

5 19. Pure zirconium is obtained using the two-step Van Arkel process. In the first step, impure zirconium and iodine are heated to produce zirconium iodide (ZrI 4). In the second step, ZrI 4 is decomposed to produce pure zirconium. ZrI 4(s) Zr(s) + 2I 2(g) Determine the percent yield of zirconium if 45.0 g ZrI 4 is decomposed and 5.00 g pure Zr is obtained. 20. A sealed flask contains neon, argon, and krypton gas. If the total pressure in the flask is atm, the partial pressure of Ne is atm, and the partial pressure of Kr is atm, what is the partial pressure of Ar in torr? 21. Hot-air balloons rise because the hot air inside the balloon is less dense than the cooler air outside. Calculate the volume an air sample will occupy inside a balloon at 43.0 o C if it occupies 2.50 L at the outside air temperature of 22.0 o C, assuming the pressure is the same at both locations. 22. A sample of nitrogen gas is stored in a ml flask at 108 kpa and 10.0 o C. The gas is transferred to a ml flask at 21.0 o C. What is the pressure of nitrogen in the second flask? 5

6 23. CO is a product of incomplete combustion of fuels. Find the volume that 42 g of CO gas occupies at STP. 24. A 2.00 L flask is filled with propane gas (C 3H 8) at 1.00 atm and o C. What is the mass of the propane in the flask? 25. When heated, solid potassium chlorate (KClO 3) decomposes to form solid potassium chloride and oxygen gas. If 20.8 g of potassium chlorate decomposes, how many liters of oxygen gas will form at STP? 26. What mass of water must be added to g NaCl to make a percent by mass aqueous solution? 27. How many grams KOH are contained in 64.3 ml M solution? 28. How many ml of M HBr solution can be made from 50.0 ml of 8.00 M HBr solution? 29. Calculate the molality of a solution that contains 15.7 g NaCl in g H 2O. 6

7 30. Calculate the freezing point and boiling point of 2.75 m NaOH in water. 31. How much heat does a 2000 kg granite boulder absorb as energy from the sun causes its temperature to change from 10 o C to 29 o C? 32. How much heat is evolved when 1255 g of water condenses to a liquid at 100 o C? 34. NO gas and Cl 2 gas react according to the equation 2NO + Cl 2 2NOCl. Use the following data to determine the rate law for the reaction by the method of initial rates. Also, calculate the value of the specific rate constant. Initial [NO] Initial [Cl 2] Initial Rate (mol/l-min) x x x

8 33. What mass of octane must be burned in order to liberate 5340 kj of heat? (ΔH comb = kj/mol) 35. The concentration of reactant A decreases from mol/l at time = 0 to mol/l at time = 4.00 min. Calculate the average reaction rate during this time period. 36. Calculate K eq for the following equilibrium when [SO 3] = M, [SO 2] = M, and [O 2] = M. heat + 2SO 3(g) 2SO 2(g) + O 2(g) 37. Predict the shift in the equilibrium of the chemical equation in #36 if: a. the volume increases b. the pressure increases c. [O 2] decreases d. [SO 3] increases e. the temperature decreases Answers: x x x x x x x , x x x x acid acid AlBr 3 Al 2S 3 bent CaCO 3 Cl C 3H 8O 3 C 5H 8NO 4Na 2C8H18 chloric CoBr 2 CO 2 16CO2 Cs 3N Cu diarsenic dinitrogen FeF 2 fourth H 2O 18H2O hydroselenic I 2 k[no] 2 [Cl2] left left Mg MnO2 Na Na 2SO 3 N 2 (NH 4) 3PO 4 nitrogen nonpolar nonpolar NR NR 25O2 octahedral planar polar polar pyramidal right right right Sb sulfur tetrafluoride tetrahedral trigonal trigonal trioxide Units: amu atoms e e formula units g g g g g g g g g kj kj kpa L L L L 2 /(mol 2 x min) p + p + m ml mol mol mol mol mol/(l x min) molecules n 0 n 0 torr oc oc % % % % % 8

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