1996 - U.S National Chemistry Olympiad 1996 Local Section...

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U.S. National Chemistry Olympiad: 1996 Local Section Test Go to Answers 1. Which gas is both diatomic and colored? (A) carbon monoxide (B) chlorine (C) nitrogen dioxide (D) oxygen 2. Which formula represents a peroxide? (A) Li 2 O (B) SiO 2 (C) Na 2 SiO 3 (D) BaO 2 3. Which statement about the halogen family is true? (A) Each of the halogens can be obtained by the electrolysis of its respective molten halide salt. (B) Iodine is the strongest oxidizing agent. (C) Bromine is obtained by oxidation using chloride ions as the oxidizing agent. (D) Halide ions are generally more reactive than the parent halogens. 4. All of these substances are important industrial reducing agents except (A) C (B) CO (C) CO 2 (D) H 2 5. What is the general formula for the alkali metal hydrides? (A) MH (B) MOH (C) MH 2 (D) M(OH) 2 6. Each of three samples was weighed on a different balance. The masses of the three are 1.028 kg, 82.9 g, and 45.1 mg. The sum of the three masses should be reported as (A) 1110.9451 g (B) 1111 g
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(C) 110 g (D) 1.11 x 10 3 g 7. Magnetite, Fe 3 O 4 , is a mixture of iron(II) oxide and iron(III) oxide. What is the most likely ratio of iron(II) oxide to iron(III) oxide in magnetite? (A) 1:1 (B) 1:2 (C) 2:3 (D) 3:2 8. A student wishes to prepare 250.mL of a 0.200 M solution of Na 2 SO 4 . Which of these procedures should be followed? Substance Molar Mass Na 2 SO 4 142 g mol¯ 1 (A) 28.4 g of Na 2 SO 4 should be dissolved in 250. mL of water in a large bottle. (B) 250. mL of water should be added to 28.4 g of Na 2 SO 4 in a large bottle. (C) 7.10 g of Na 2 SO 4 should be dissolved in enough water to fill a graduated beaker to the 250. mL mark. (D) 7.10 g of Na 2 SO 4 should be dissolved in a small amount of water and diluted to 250. mL in a volumetric flask. 9. How many moles of ozone, O 3 , could be formed from 48.0 g of oxygen gas, O 2 ? (A) 1.00 mol (B) 1.30 mol (C) 1.50 mol (D) 2.00 mol 10. How many grams of carbon are present in 0.50 mol of sucrose (C 12 H 22 O 11 )? Substance Molar Mass C 12 H 22 O 11 342 g mol¯ 1 (A) 60 g (B) 72 g (C) 90 g (D) 120 g
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11. If excess Ca(OH) 2 is treated with 0.160 mol of dry HCl gas, what is the maximum number of grams of CaCl 2 that could be formed? Substance Molar Mass Ca(OH) 2 74.1 g mol¯ 1 HCl 36.5 g mol¯ 1 CaCl 2 111.0 g mol¯ 1 (A) 35.5 g (B) 17.8 g (C) 8.88 g (D) 4.44 g 12. What volume of 0.500 M CaCl 2 solution is needed to prepare 250 mL of solution that has a chloride concentration of 0.100 M? (A) 12.5 mL (B) 25.0 mL (C) 50.0 mL (D) 100 mL 13. Which group II element would be expected to be the hardest? (A) Be (B) Mg (C) Ca (D) Ba 14. Chlorine reacts with fluorine above 200 °C to form chlorine trifluoride, ClF 3 , as shown by this equation: Cl 2 (g) + 3F 2 (g) ---> 2ClF 3 (g) If equal numbers of moles of chlorine and fluorine are combined, the maximum number of moles of ClF 3 that could be formed will be equal to (A) the number of moles of Cl 2 . (B) the number of moles of F
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This note was uploaded on 11/09/2011 for the course CHEM 111 taught by Professor Rogers during the Fall '08 term at Thomas Edison State.

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1996 - U.S National Chemistry Olympiad 1996 Local Section...

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