Chem Midterm 21 Review Key

University:
University of North Georgia
Course:
CHEM 1211 | Principles of Chemistry I
Academic year:

2022
Views:

254

Pages:

3
Author:

larbiwxcvbn

Part A: Inorganic Chemistry Name the following compounds: Chlorine dioxide: ClO₂ Silicon hexafluoride: SiF₆ Dihydrogen dioxide: H₂O₂ Aluminum sulfide: Al₂S₃ Aluminum sulfate: Al₂(SO₄)₃ Calcium phosphate: Ca₃(PO₄)₂ Calcium phosphide: Ca₃P₂ Boron triiodide: BI₃ Iron(II) oxide: FeO Dinitrogen pentoxide: N₂O₅ Cobalt(I) carbonate: Co₂CO₃ Beryllium iodide: BeI₂ Part B: Organic Chemistry 1. Draw the following molecules: Heptane: C-C-C-C-C-C-C Ethane: C-C 2-ethyl, 3-methylpentane: C | C-C-C-C-C | C 2,2-dimethylbutane: C | C-C-C-C | C Pentane: C-C-C-C-C 3,3-diethyl, 2,4-dimethylheptane: C | C-C-C-C-C-C-C | | | C C C 2. Write the names of the following molecules: CH₃(CH₂)₅CH₃: heptane CH₃CH₃: ethane Part B: Organic Chemistry 1. Draw the following molecules: 2,2,3-trimethylpentane C | C-C-C-C-C | | C C 3-propylheptane C-C-C-C-C-C-C | C-C-C 2,3-diethylpentane C-C-C-C-C | | C C 3. What is an isomer? Two molecules with the same molecular formula but different structural formulas. 4. Draw 2 isomers for octane C-C-C-C-C-C-C-C C-C(C)-C-C(C)-C-C Part 9: The Mole 1. 1 mole = 6.02 x 10^23 representative particles 2. What is the molar mass of each of the following: a) Al₂(SO₄)₃: 342.17 g/mol b) C₆H₁₂O₆: 180.18 g/mol c) AgNO₃: 169.88 g/mol d) N₂O₅: 108 g/mol e) O₂: 32 g/mol f) MgCl₂: 95.21 g/mol 3. How many grams of CO₂ are in 0.56 moles of carbon dioxide? 0.56 mol CO₂ * (44 g CO₂ / 1 mol CO₂) = 24.64 g CO₂ 4. What is the mass, in grams, of 6.7 x 10^23 atoms of aluminum (Al)? 6.7 x 10^23 atoms Al * (1 mol Al / 6.02 x 10^23 atoms Al) * (26.98 g Al / 1 mol Al) ≈ 30.03 g Al Part 9: The Mole 5. How many atoms are in 1.4 moles of sodium (Na)? 1.4 mol Na * (6.02 x 10^23 atoms Na / 1 mol Na) = 8.43 x 10^23 atoms Na 6. What is the percent composition of: a) AgNO₃ (Molar mass: 169.88 g/mol) Ag: (107.87 / 169.88) * 100 = 63.50% N: (14.01 / 169.88) * 100 = 8.25% O: (3 * 16 / 169.88) * 100 = 28.26% b) Al₂(SO₄)₃ (Molar mass: 342.17 g/mol) Al: (2 * 26.98 / 342.17) * 100 = 15.77% S: (3 * 32.07 / 342.17) * 100 = 28.12% O: (12 * 16 / 342.17) * 100 = 56.11% 7. What is the empirical formula of: a) C₆H₁₂O₆ CH₂O b) N₂O₅ N₂O₅ 8. What is the molecular formula of a compound whose molar mass is 90 g/mol and empirical formula is CH₂O? CH₂O x n = 90 30 x n = 90 n = 3 C₃H₆O₃ 9. Find the empirical formula of a compound containing 25.9% nitrogen and 74.1% oxygen. 25.9 g N * (1 mol N / 14 g N) = 1.85 mol N 74.1 g O * (1 mol O / 16 g O) = 4.63 mol O 1.85 / 1.85 = 1 x 2 = 2 4.63 / 1.85 = 2.5 x 2 = 5 N₂O₅ Part 10: Stoichiometry Use the equation above for the next 3 Stoichiometry problems: 2H₂S + 3O₂ → 2SO₂ + 2H₂O 1. If we start with 60g H₂S and excess O₂, how many grams of H₂O will be produced? 60 g H₂S * (1 mol H₂S / 34.08 g H₂S) * (2 mol H₂O / 2 mol H₂S) * (18.02 g

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