TAME Math and Science Contest
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- Susanna Horton
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1 Answer the following questions by marking the BEST answer on the answer sheet. 1. What is the order of increasing energy for the four orbitals 4s, 2p, and 3d in the neutral calcium atom? a. 2p < 3p < 3d < 4s b. 4s < 3d < 3p < 2p c. 2p < 3p < 4s < 3d d. 4s < 2p < 3p < 3d e. 3p < 2p < 4s < 3d 2. Which of the following would have a Lewis structure most like that of CO 2-3 a. O 3 b. CO 2 c. C 2 O 3 d. NO 3 1- e. SO The reaction CaO (s) + H 2 O (l) Ca (OH) 2 (s) is spontaneous at 25 C and the reverse reaction is spontaneous at some high temperature. This means that a. ΔH >0, ΔS>0. b. ΔH<0, ΔS>0. c. ΔH>0, ΔS=0. d. ΔH>0,ΔS<0. e. ΔH<0, ΔS<0. 4. If you inflated a balloon at sea level where the pressure is 29.7 inches of Hg and then carried it to a mountain top, where the pressure is 18.3 inches of Hg, by what factor would the volume of the balloon change? (Assume a constant pressure.) a. 29.7/18.3 b. ( )/29.7 c. ( )/18.3 d. 18.3/29.7 e. 1.0 (no change) 5. In an electric fuel cell using the reaction CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O (l) a. chemical energy is converted directly to electrical work. b. carbon is reduced. c. oxygen is oxidized. d. CH 4 and O 2 both react a the same electrode. e. oxygen is the catalyst for the reaction. 6. A substance is a blue crystalline solid at 25 C and decomposes at 300 C to give a white powdery solid and another volatile product. The blue solid dissolves in water to give a conducting solution. What is the blue solid? a. CuSO 4 b. CuSO 4 5H 2 O c. Cu d. Cu 2 S e. an alloy of Cu & Ag 7. One gram of which of the following contains the largest number of molecules? a. CH 4 b. NH 3 c. HNO 3 d. N 2 e. H 2 O 8. A particular radioactive series starts with 235 U and ends with the stable 207 Pb. In the overall process, how many alpha and beta particles are emitted? a. 8 alpha, 6 beta b. 14 alpha, 10 beta c. 7 alpha, 10 beta d. 8 alpha, 10 beta e. 7 alpha, 4 beta 9. The total number of structurally isomeric alcohols with the formula C 4 H 9 OH is a. one b. two c. three d. four e. five 10. Approximately stoichiometric amounts of reactants are allowed to react. Given sufficient time to reach equilibrium, the reaction will go to completion (that is, the reactions will be almost entirely converted to products) if (K is the equilibrium constant)? a. K is very small. b. K is much larger than one. c. K is much closer to one. d. ΔG = 0. e. ΔG is a large positive number. Released 2007 Page 1 of 6
2 11. Which of the following slightly soluble salts would not be soluble in a strong acid (like HClO 3 )? a. PbCO 3 b. CaF 2 c. PbSO 4 d. Ag 3 PO 4 e. AgC 2 H 3 O The effectiveness of a catalyst depends on its ability to a. increase the equilibrium constant. b. decrease the activation energy. c. decrease the free energy change. d. increase the reactant concentrations. e. increase the temperature. 13. Which of the following species is diamagnetic? a. NO b. NO 2 c. CO + d. CO 2 e. CH What types of hybridization are used by carbon atoms in methyl acetylene? a. sp only b. sp and sp 2 c. sp 2 and sp 3 d. sp 3 only e. sp and sp ΔH for the reaction Cl 2 2Cl (all gasses) is: a. -58 kcal. b kcal. c. 0.0 kcal. d. +58 kcal. e. -2 kcal. 16. Two flasks are filled with different gases. One holds 0.48g of ozone, O 3. The other flask is twice the volume of the first and holds 0.68g of an unknown gas. The two gases are at the same temperature and pressure. What is the unknown gas? a. H 2 S b. SO 2 c. O 2 d. C 5 H 8 e. O The average oxidation number of nitrogen atoms in hydrazoic acid, HN 3, is a. -3. b. -1. c. -1/3. d. +1. e The process by which a metal sulfide ore is converted to the metal or to an oxide by heating in air is called a. combustion. b. flotation. c. reduction. d. roasting e. aggregation. 19. Experimental support for the arrangements of electrons in distinct energy levels is primarily based upon a. the law of constant composition. b. the discrete spectra of gaseous electrical discharges. c. the law of conservation of energy. d. the law of multiple proportions. e. the law of DuLong and Petit. 20. Which of the following are correct Lewis structures for C 2 H 4 O? I) H 2 C CH 2 II) CH3 -- C = O III) CH 2 = C -- O -- H H H O a. I b. II and III c. II d. III e. all of them 21. Analysis of a gaseous mixture of NO and N2O shows that it contains 52% by weight of nitrogen. What is the percent by weight of NO in the mixture? a. 55.7% b. 88.6% c. 68.6% d. 52.0% e. 36.6% 22. When 500mL of 0.10 M NaOH is reacted with 500mL HCl, the final H + concentration is about a M. b M. c M. d M. e M. Released 2007 Page 2 of 6
3 23. A 5.0 L flask holds a mixture of NO and C 3 H 6 at 27 C and a total pressure of 1.50 atm. Analysis shows that the flask holds 2.10g of C 3 H 6. What is the partial pressure of NO? (R = L atm / mol K) a atm b atm c atm d atm e atm 24. The standard free energy of formation of AgBr (s) is 22.9 kcal/mol. What is the standard potential of a cell with the overall reaction: (Faraday constant: F = kcal / volt) 2 Ag + Br 2 2 AgBr (s) E =? a v b v c v d v e v 25. A 0.946g sample of a compound is dissolved in 150g of water to give a solution with a freezing point of C. What is the molecular weight of the compound? (K f = 1.86 deg / molal) a. 180 b. 150 c. 97 d e The hydrogen atom energy levels are given by E = -R H /n 2, where R H = 2.18 x joule. What is the wavelength of the second Lyman transition (n = 3 to n = 1). (h = 6.63 x j sec; c = 3 x 10 8 m/sec) a x m b x 10-5 m c x 10-7 m d x 10-7 m e x m 27. For the reaction 2 HI H 2 + I 2, K c = How many moles of I 2 are there at equilibrium, starting with 0.30 mole of HI? a b c d e. No solution possible: volume of container not given. 28. When acetylene (C 2 H 2 ) burns in air, the products are CO 2 and H 2 O (l). If one mole of C 2 H 2 is burned with 64.0g of O 2, what is the theoretical yield of CO 2? a g b. 176 g c g d g e g 29. Which has the highest percentage of oxygen? a. NaHCO 3 b. (NH 4 ) 2 SO 4 c. Na 2 S 2 O 3 d. H 2 O Arrange the following in order of increasing mass: w. 1 molecule of I 2 x. 4.0 x molecules of C 4 H 10 y x molecules of CO z. 1 mole of P 2 O 5 a. w, y, x, z b. y, w, z, x c. z, x, y, w d. x, y, w, z 31. Several groups of students from Texas High were hired by Polymer Company, Inc. to mass 33.0 g of a sample of sodium thiosulfate. Their data is listed below. Group A: 35.2 g 35.3 g 35.3 g 35.2 g Group B: 33.5 g 33.5 g 33.4 g 33.5 g Group C: 40.5g 53.5 g 35.3 g 30.2 g Which group of students had good Precision and poor Accuracy? a. Group A b. Group B c. Group C 32. Sodium tetraborate, Na 2 B 4 O 4, is produced according to the unbalanced equation: H 3 BO 3 + NaOH H 2 O + Na 2 B 4 O 7 How many grams of Boric acid, H 3 BO 3, are needed to make 150,000 grams of Na 2 B 4 O 7? a grams b x 10-3 c grams d grams Released 2007 Page 3 of 6
4 Solubility (grams per 100 grams of water TAME Math and Science Contest 33. Magnesium can be reacted with Iodine to form magnesium iodide. How many grams of magnesium iodide can be formed from 8.06 grams magnesium and grams iodine? a. 75.5grams b grams c grams d grams For questions use the solubility graph below. Solubilities NaNO 3 KNO NaCl Yb 2 (SO 4 ) Temperature (C degrees) 34. According to the solubility graph, at 30 C, which of the following compounds is the most soluble in 100 grams of water? a. NaCl b. Yb 2 (SO 4 ) 3 c. KNO 3 d. NaNO According to the graph, 110 grams of KNO 3 dissolves at what temperature? a. 30 C b. 40 C c. 60 C d. 70 C 36. The molarity of a solution in which 15.5g NaOH is dissolved in 0.100L of solution is? a. 620 M b M c M d M 37. How many grams of ZnCl 2 are needed to make 25.0 ml of M ZnCl 2 solution? a g b g c. 2.6 g d. 4.2 g Released 2007 Page 4 of 6
5 38. What is the percent composition of sulfur by mass in this sample: 64 g S and 152 g Na? a. 29.6% b. 42.1% c % d. 70.3% 39. What is the percent composition of hydrogen by mass in C 3 H 8? a % b. 82% c. 50.0% d. 72.0% 40. The following equation can be balanced with which set of coefficients? Fe 2 O 3 + CO CO 2 + Fe a. 1, 2, 4, 3 b. 3, 3, 2, 1 c. 2, 3, 3, 2 d. 1, 3, 3, 2 e. 1.3, 3, 3 END OF TEST Released 2007 Page 5 of 6
6 Answer Key 1. C 2. D 3. E 4. A 5. A 6. B 7. A 8. E 9. D 10. B 11. C 12. B 13. D 14. E 15. D 16. A 17. C 18. D 19. B 20. E 21. C 22. E 23. B 24. C 25. A 26. D 27. D 28. A 29. D 30. C 31. A 32. D 33. C 34. D 35. C 36. B 37. B 38. A 39. A 40. D Released 2007 Page 6 of 6
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