Chem1310_Exam1_practice-1 - Chem 1310; Exam 1 Name: _ Lab...

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Chem 1310; Exam 1 Name: _________________________________________ Lab Section: 1. When 3.0 L of hydrogen gas (H 2 ) reacts with 2.0 L of nitrogen gas (N 2 ), 2.0 L of gaseous product are formed. All volumes of gases are measured at the same temperature and pressure. What is the formula of the product? A) N 2 H 6 B) NH 3 C) NH 4 D) NH E) N 2 H 3 2. Which of the following is not the correct chemical formula for the compound named? A) N H 4 OH 2 ammonium hydroxide B) K CN potassium cyanide C) F e 3 O 2 ir on(III) oxide D) B aS barium sulfide E) M g(C 2 H 3 O 2 ) 2 magnesium acetate 3. For one element, 90.51% is an isotope with mass 19.992 amu, 0.270% is an isotope with mass 20.994 amu, and 9.22% is an isotope with mass 21.990 amu. Calculate the average atomic mass and identify the element. A) 20.2, Ne B) 20.2, F C) 21.0, Ne D) 21.0, Na E) none of the above 4. Ferrocene has the formula Fe(C 5 H 5 ) 2 . The number of moles of ferrocene in 100.0 g of f errocene is A) 2.703 B) 0.5375 C) 0.8269 D) 1.074 Page 1
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Name: _________________________________________ 5. Iron is produced from its ore by the reactions: 2C(s) + O 2 (g) 2CO(g) Fe 2 O 3 (s) + 3CO(g) 2Fe(s) + 3CO 2 (g) How many moles of O 2 (g) are needed to produce 1 mole of Fe(s)?
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This note was uploaded on 07/07/2009 for the course CHEM 1310 taught by Professor Cox during the Spring '08 term at Georgia Institute of Technology.

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Chem1310_Exam1_practice-1 - Chem 1310; Exam 1 Name: _ Lab...

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