Final_Study_Guide_Spring_2009_-_KEY[1]

Final_Study_Guide_Spring_2009_-_KEY[1] - Chemistry 1 Final...

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Chemistry 1 Final Exam Study Guide Spring 2009 1. If a substance has a mass of 36.4 g and a volume of 8.500 mL, what is its density? 4.28 g/mL 2. Which involves a chemical change? a. powdering sugar b. condensing steam c. magnetizing an iron bar d. separating cream from milk e. exposing photographic film to light 3. Describe the following separation techniques. a. filtration uses a porous barrier to separate a solid from a liquid on the basis of particle size b. distillation used to physically separate homogeneous mixtures based on the differences in substances’ boiling points c. chromatography used to separate parts of a mixture based on their tendencies to travel across the surface of another material. Some compounds are more soluble in the mobile phase; others adhere strongly to the stationary phase. 4. During an experiment, a student found the concentration of an aqueous sucrose solution to be 2.368 M. If the actual concentration of the solution is 2.450 M, what is the student’s percent error? 3.347% 5. Complete the following chart for the 6 phase changes. Phase Change Initial Phase Final Phase Endothermic or Exothermic? Vaporization Liquid Gas Endo Sublimation Solid Gas Endo Freezing Liquid Solid Exo Deposition Gas Solid Exo Melting Solid Liquid Endo Condensation Gas Liquid Exo
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6. How do atmospheric pressure and the vapor pressure of a substance relate to the boiling point of the substance? Vapor pressure of a liquid increases with temperature. Atmospheric pressure and a substance’s vapor pressure are equal at the boiling point of that particular substance. 7. What is correct formula for nickel (II) nitrate? a. NiNO 2 b. Ni(NO) 3 c. Ni 2 NO 3 d. Ni(NO 3 ) 2 8. How many liters of methane gas (CH 4 ) at STP are there in 3.67 x 10 24 molecules? a. 58.7 L b. 137 L c. 97.5 L d. 218 L 9. Name the following compound: FeSO 4 •6H 2 O. What is its molar mass? Iron (II) sulfate hexahydrate; 259.92 g/mol 10. If you have one mole samples of silver (Ag), gold (Au), and platinum (Pt), which quantity will be the same for all of the samples? a. volume b. density c. monetary value of metals d. number of atoms e. mass 11. What is the percent by mass of magnesium in magnesium chloride? a. 68.5% b. 34.2% c. 25.5% d. 50.0% 12. Write a balanced equation for a reaction between NaOH and CuCl 2 . 2 NaOH + CuCl 2 2 NaCl + Cu(OH) 2 13. Balance the following equation: _ 3 _ Ca(OH) 2 + _ 2 _ H 3 PO 4 → ___ Ca 3 (PO 4 ) 2 + _ 6 _ H 2 O 14. Calculate the mass of CO 2 formed from the combustion of 25 grams of methane: CH 4 + 2O 2 CO 2 + 2H 2 O 69 g
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15. Citric acid (H 3 C 6 H 5 O 7 ) is a product of the fermentation of sucrose (C 12 H 22 O 11 ) in air. C 12 H 22 O 11 + 3 O 2 2 H 3 C 6 H 5 O 7 + 3 H 2 O Determine the number of moles of citric acid produced when 2.50 moles of sucrose reacts. 5.00 mol
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Final_Study_Guide_Spring_2009_-_KEY[1] - Chemistry 1 Final...

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