Syracuse University Project Advance s1

Chemistry 106: General Chemistry Syracuse University Project Advance Final Exam, Fall 2004

Name Date

The last page of each examination is a periodic table.

c = 3.00 x 108 m/sec h = 6.63 x 10-34 Js -24 mp = 1.67 x 10 g (mass of proton) -18 Rydberg Constant (RH) = 2.18 x 10 J

(1) What is the volume of a 12.2 g piece of metal with a density of 9.43 g/cm3?

(a) 12.2 cm3 (b) 1.29 cm3 (c) 0.773 cm3 (d) 115 cm3 (e) none of these

(2) Which of the following values contains 2 significant figures?

(a) 0.0004 kg (b) 0.0040 L (c) 0.0400 mm (d) 0.4000 m (e) all of these

(3) All atoms of a given element have the same

(a) mass (b) number of neutrons (c) number of protons (d) same ratio of protons and neutrons (e) there is nothing constant about a given element

(4) When a metal and a non metal react, the tends to lose electrons, and the tends to gain electrons

(a) metalloid, metal (b) nonmetal, nonmetal (c) metal, nonmetal (d) nonmetal, metal (e) none of these, these elements share electrons

(5) What is the chemical formula for iron(III) sulfide?

CHE 106 1 Fall 2004 Final Exam (a) Fe2(SO3)3 (b) Fe2S3 (c) Fe3(SO3)2 (d) Fe2(SO4)3 (e) Fe3(SO4)2

(6) What is the percentage of Ca (by weight) in Ca3(PO4)2?

(a) 9.9% (b) 20.0% (c) 18.7% (d) 38.8% (e) 55.9%

(7) What is the empirical formula of caffeine if it contains 5.19% H, 28.85% N, 16.48% O, and 49.48% C by weight?

(a) C10HN5O3 (b) C4H5NO2 (c) C3H5NO (d) C2H6NO2 (e) C4H5N2O

(8) What is the mass of copper produced if 10.0 g of Cu2S reacts with 16.0 g of O2 as follows: (Atomic masses are Cu = 63.5; O = 16.0; S = 32.1)

Cu2S + O2  2 Cu + SO2 (a) 31.8 g (b) 63.5 g (c) 3.99 g (d) 7.98 g (e) 6.25 g

21 (9) One gram of TNT, C7H5N3O6, has 7.95 x 10 nitrogen atoms. How many hydrogen atoms are there in 1.00 g of TNT? (a) 7.95 x 1021 (b) 9.26 x 1021 (c) 1.33 x 1022 (d) 1.59 x 1022 (e) 1.86 x 1022 (10) How many grams of carbon dioxide (CO2, molar mass = 44.0 g/mol) are produced in the combustion of 1.8 g glucose (C6H12O6, molar mass = 180.0 g/mol) according to the following reaction: CHE 106 2 Fall 2004 Final Exam C6H12O6(g) + 6 O2(g)  6 CO2(g) + 6 H2O (g) ?

(a) 1.08 g (b) 0.440 g (c) 4.40 g (d) 0.264 g (e) 2.64 g

(11) A space explorer traveling to a distant planet in the universe found an element X whose 2 isotopes had the approximate masses and percentage abundances 140. amu (66.7%) and 143. amu (33.3%). What is the average relative atomic mass of 1 2 element X on that planet as compared with 6 C taken as 12 amu?

(a) 140. amu (b) 140.6 amu (c) 141. amu  (d) 141.6 amu (e) 142. amu

(12) Balance the following equation: __Cl2O7 + __H2O  __HClO4 The ratio of the coefficient of HClO4 to the coefficient of H2O is

(a) 1/2 (b) 2/3 (c) 1/1 (d) 3/2 (e) 2/1

(13) You want to prepare 250 mL of 0.10 M Na2SO4 (aq). The molar masses of H2O and Na2SO4 are 18.02 g/mol and 142.04 g/mol respectively. The mass of Na2SO4 required is

(a) 0.451 g (b) 3.55 g (c) 3550 g (d) 0.000176 g (e) 0.176 g

(14) How many ml of 0.100 M H2SO4 are required to react with 0.840 g of NaHCO3 (molar mass = 84.01 g/mol) according to the following equation?

H2SO4(aq) + 2NaHCO3(aq)  Na2SO4(aq) + 2H2O(l) + 2CO2(g) (a) 200 mL CHE 106 3 Fall 2004 Final Exam (b) 150 mL (c) 100 mL (d) 50.0 mL (e) none of the above

(15) Obtain the oxidation number for the element noted in each of the following:

- I. N in NH2 - II. I in IO3 - III. Al in Al(OH)4 Add together the results of I, II and III. The sum is (a) -3 (b) -1 (c) +1 (d) +3 (e) +5

(16) Consider the oxidation-reduction reaction:

2FeI3(aq) + 3Mg(s)  2Fe(s) + 3MgI2(aq).

Which of the following statements is not true about this reaction? (a) Iron (Fe) acts as an oxidizing agent. (b) Magnesium (Mg) acts as a reducing agent. (c) The oxidation number of iron is lowered. (d) The oxidation number of Mg is lowered. (e) Iodide ion (I-) is a spectator ion.

(17) How many moles of sulfate ions are there in a 0.20 L solution of 0.030 molar Al2(SO4)3?

(a) 0.0030 (b) 0.0060 (c) 0.012 (d) 0.018 (e) 0.024

(18) Calculate the standard heat of formation of acetaldehyde, CH3CHO(g), given the following information:

5 CH3CHO(g) + O2(g)  2H2O(l) + 2CO2(g) H = -1194 kJ 2 Hf° H2O(l) = -286 kJ/mol Hint: Write out Hf equations for H2O and CO2 CHE 106 4 Fall 2004 Final Exam  Hf° CO2(g) = -394 kJ/mol

(a) -452 kJ (b) -332 kJ (c) -166 kJ (d) 166 kJ (e) 332 kJ

(19) Hfus for sulfur is 17.7 kJ/mol. How many grams of sulfur can be melted by 29.0 kJ of energy? (a) 9.8 g (b) 19.5 g (c) 26.2 g (d) 40.7 g (e) 52.5 g

(20) Given the following data at 25°C and 1.00 atm pressure:  H°(kJ/mol)

Pb(s) + PbO2(s) + 2H2SO4(l)  2PbSO4(s) + 2H2O(l) -509.2

SO3(g) + H2O(l)  H2SO4(l) -130

Evaluate H° for the reaction below at 25°C.

Pb(s) + PbO2(s) + 2SO3(g)  2PbSO4(s) (a) -3.77 x 103 kJ (b) 3.77 x 103 kJ (c) -639 kJ (d) -521 kJ (e) -769 kJ

(21) Calculate the standard enthalpy change of the reaction of the combustion of propane:

C3H8(g) + 5O2(g)  3CO2(g) + 4H2O(l)

Use the following data:  Hf° (kJ/mol)

CHE 106 5 Fall 2004 Final Exam C3H8(g) -103.8 CO2(g) -393.5 H2O(g) -285.8

(a) +575.5 kJ (b) -575.5 kJ (c) -2428. kJ (d) +2200. kJ (e) -2200. kJ

(22) The possible value(s) of the magnetic quantum number m1 for a 5d electron is(are) (a) 0, 1, 2, 3 (b) 1, 2, 3, 4 (c) 2, 1, 0, -1, -2 (d) 3, 2, 1, 0, -1, -2, -3 (d) 4

(23) What is the electron configuration of Fe+3?

(a) [Ar] 3d64s2 (b) [Ar] 3d34s2 (c) [Ar] 3d44s1 (d) [Ar] 3d5 (e) [Ar] 3d6

(24) In the Periodic Table, Mg is in Group IIA and Period 3, Ca is in Group IIA and Period 4, and S is in Group VIA and Period 3. Arrange these elements in order of increasing ionization energy.

(a) Mg Ca S (b) Mg S Ca (c) Ca Mg S (d) S Ca Mg (e) S Mg Ca

(25) London-dispersion force is the attractive force between (a) an ion and a permanent dipole (b) an instantaneous dipole and an induced dipole (c) two permanent dipoles (d) two molecules with hydrogen bonds to an oxygen atom (e) two ions

(26) Write the Lewis Electron Dot Formula of [ClO]-. Which of the following statements is/are incorrect?

I. The total number of valence electrons is 14.

II. The skeleton structure is Cl-O.

III. The best Lewis formula is C l = O (a) III CHE 106 6 Fall 2004 Final Exam (b) II (c) I (d) I and II (e) II and III

(27) The octet rule is violated by at least one atom in each of the following species except

- (a) ICl2 . - (b) CH3 . - (c) BF4 . (d) SF4. (e) ClF3.

(28) A  (pi) bond is the result of the

(a) overlap of an s orbital and a p orbital. (b) overlap of two p orbitals along their axes. (c) overlap of two s orbitals. (d) sidewise overlap of two s orbitals. (e) sidewise overlap of two parallel p orbitals.

(29) The hybridization of the central atom in a molecule is described as sp. The arrangement in space of the hybrid orbitals about that atom is

(a) linear. (b) trigonal planar. (c) tetrahedral. (d) trigonal bipyramidal. (e) octahedral.

(30) During lecture a chemistry student inflates five identical balloons with the gases below to a volume of 1 liter at 298 K and a pressure of 1 atm. The student continues to observe the balloons for a long period of time, and notices that one decrease in size. According to Graham’s law, which balloon would shrink over time? (Air = 79% N2, 21% O2)

(a) The balloon filled with CO2. (b) The balloon filled with H2. (c) The balloon filled with NO2. (d) The balloon filled with Ar. (e) The balloon filled with SF6. CHE 106 7 Fall 2004 Final Exam (31) The volume of a sample of gas measured at 25.0°C and 1.00 atm pressure is 10.0 L. What must the final temperature be in order for the gas to have a final volume of 7.5 L at 1.00 atm pressure?

(a) -55°C (b) -50°C (c) -45°C (d) -35°C (e) 19°C

(32) Magnesium metal reacts with hydrochloric acid to produce hydrogen gas, H2

according to the following reaction: Mg(s) + 2HCl(aq)  MgCl2(aq) + H2(g). Calculate the volume (in liters) of hydrogen produced at 28°C and 665 mm Hg from 0.0840 mol Mg and excess HCl. (a) 1.82 L (b) 2.37 L (c) 0.220 L (d) 0.169 L (e) None of the above

(33) Based on molecular mass and dipole moment of five compounds in the table below, which should have the highest boiling point?

Compound Molecular Mass (amu) Dipole Moment (debye)

CH3CH2CH3 44 0.0 CH3OCH3 46 1.3 CH3Cl 50 2.0 CH3CHO 44 2.7 CH3CN 41 3.9

(a) CH3CH2CH3 (b) CH3OCH3 CHE 106 8 Fall 2004 Final Exam (c) CH3Cl (d) CH3CHO (e) CH3CN

CHE 106 9 Fall 2004 Final Exam