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Name: _____________________________ Per: ____ CHEMISTRY: Practice Spring Final MRS. WARD Note: Do not JUST study this practice exam; it does not contain every topic that may appear on your final exam. Be sure to look at your review guide to see a list of topics you are responsible for. Also, this practice test is broken up by topic; your final exam will not be. CHEMICAL REACTIONS 1) Classify the following reaction: 3CuSO4 + 2Al Al2(SO4)3 + 3Cu A) synthesis C) double replacement B) single replacement D) decomposition 2) Classify the following reaction: Cu(OH)2 CuO + H2O A) synthesis C) double replacement B) single replacement D) decomposition 3) What is the balanced equation when aluminum reacts with copper II sulfate? A) Al + Cu2S Al2S + Cu C) Al + CuSO4 AlSO4 + Cu B) 2Al + 3CuSO4 Al2(SO4)3 + 3Cu D) 2Al + Cu2SO4 Al2SO4 + 2Cu 4) In a combustion reaction, one of the reactions is A) hydrogen C) oxygen B) nitrogen D) a metal 5) Balance the following equation: Fe + O2 Fe2O3 A) 4, 3, 2 C) 1, 2, 3 B) 2, 1, 1 D) 2, 3, 1 6) Which one of the following metals could produce zinc metal, if heated with zinc oxide? A) Aluminum B) Copper C) Iron D) Silver 7) A compound contains 6.0 g of cabon and 1.0 g of hydrogen. The percent composition of the compound is: A) 14 % hydrogen and 86 % carbon B) 86 % hydrogen and 14 % carbon C) 17 % hydrogen and 83 % carbon D) 83 % hydrogen and 17 % carbon STOICHIOMETRY 8) The molecular formula for aspirin is C9H8O4. What is its empirical formula? A) C9H8O4 B) C3H2O2 C) CHO D) none of the above 9) What is the empirical formula for a compound that is 31.9% potassium, 28.9% chlorine, and 39.2% oxygen? A) KClO2 B) KClO3 C) K2Cl2O3 D) K2Cl2O5 10) A compounds empirical formula is NO2. If the molar mass is 92 g/mol, what is its molecular formula? A) NO B) N2O2 C) NO2 D) N2O4 11) What is the number of moles in 500 L of He gas at STP? A) 0.05 mol B) 0.2 mol 12) Given the reaction: CH4 + 2 O2 1 mole of CH4? A) 2 moles C2H4 + 3 O2 B) 2 atoms C) 22 mol D) 90 mol CO2 + 2 H2O, what amount of oxygen is needed to completely react with C) 2 grams D) 2 molecules 2 CO2 + 2 H2O 13) If 6.0 mol of CO2 are produced, how many moles of O2 were reacted? A) 2.0 mol B) 6.0 mol C) 9.0 mol D) 18.0 mol 14) If 22.0 g of CO2 are produced, how many grams of H2O are produced? A) 5.50 g B) 9.00 g C) 18.0 g D) 22.2 g 15) What mass of ZnCl2 can be prepared from the reaction of 3.27 grams of zinc with 3.30 grams of HCl? Zn +2HCl A) 6.89 g ZnCl2 + H2 B) 6.82 g C) 6.46 g D) 6.17 g GASES 16) Calculate the new pressure of helium gas in a balloon if the original volume of 2.5 L at 100.0 kPa increases to 18 L. A) 0.45 kPa B) 720 kPa C) 14 kPa D) 13 kPa 17) Which of the following is not a basic assumption of kinetic theory? A) Gases are composed of particles. B) The particles of all move at the same speed C) The particles of gases are in constant motion. D) All collisions of the gas particles are perfectly elastic. 18) If the pressure of a sample of gas increases by a factor of 4, what would happen to the temperature? A) increase by a factor of 2 C) increase by a factor of 4 B) decrease by a factor of 2 D) decrease to ¼ the original temperature 19) A sample of oxygen occupies 47.2 liters under a pressure of 1240 torr at 25oC. What volume would it occupy at 25oC if the pressure were decreased to 730 torr? A) 27.8 L B) 29.3 L C) 32.3 L D) 80.2 L 20) A sample of nitrogen occupies 5.50 liters under a pressure of 900 torr at 25oC. At what temperature will it occupy 10.0 liters at the same pressure? A) 32oC B) -109oC C) 154oC D) 269oC 21) A real gas most closely approaches the behavior of an ideal gas under conditions of: A) high P and low T (C) low P and T B) low P and high T (D) high P and T 22) If there is 36 g of water vapor present at STP, what volume is present? A) 45 L B) 806 L C) 0.089 L D) 1.6 L THERMODYNAMICS 23) Two reagents are mixed in a flask. The bottom of the flask feels cold. This is an example of what kind of reaction? A) endothermic C) isothermic B) exothermic D) nucleothermic 24) How many kJ of heat is absorbed when 2.0 kg of liquid water is heated from 18oC to 85oC? (SPECIFIC HEAT WATER = 4.18 J/goC) A) 0.56 kJ B) –0.56 kJ C) 560 kJ D) 280 kJ 25) A mass of 12 g of a substance absorbs 115 J of heat. The initial temperature was 23.5 oC. After absorbing the heat, the temperature reads 35 oC. What is the specific heat capacity of the substance? A) 0.16 J/g oC C) 0.27 J/g oC B) 0.83 J/g oC D) 0.38 J/g oC 26) 4Al (s) + 3O2 (g) ¬ 2Al2O3 (s) ∆H = -3351 kJ is __________, and therefore heat is __________ by the reaction. A) exothermic, released C) endothermic, released B) exothermic, absorbed D) endothermic, absorbed 27) Which metal requires the most energy to raise 1.00 g of it by 1.00ºC? (Specific heat capacities: Al: 0.900 J/goC, Cu: 0.385 J/goC, Pb: 0.128 J/goC, Ni: 0.440 J/goC) A) aluminum B) copper C) lead D) nickel 28) What happens to the water in a calorimeter when an exothermic reaction occurs in it? A) It absorbs heat, and a drop in temperature is observed. B) It absorbs heat, and a rise in temperature is observed. C) It releases heat, and a drop in temperature is observed. D) It releases heat, and a rise in temperature is observed. SOLUTIONS 29) What is the molarity of a solution prepared by mixing 7.0 moles of NaCl in 585 mL of solution? A) 0.081 M C) 4.0 M B) 81 M D) 12 M 30) The substance that is dissolved when a solution is prepared is called A) solvent B) excess reagent C) solute D) reactant 31) What mass (in grams) of sucrose, C12H22O11, is needed to make 500.0 mL of a 0.200 M solution? A) 68.4 g B) 34.2 g C) 100 g D) 17.1 g 32) If 2.0 mL of 6.0 M HCl is used to make a 500.0-mL solution, what is the concentration of the dilute solution? A) 0.24 M B) 0.30 M C) 0.024 M D) 0.83 M 33) What is the volume of a solution that has been diluted to .5 M if the original solution was 2M and 500 mL? (A) 500 mL (C) 2000 mL (B) 100 mL (D) 50 mL 34) You are asked to prepare 500.0 mL of a 2.00 M solution of NaOH. How many grams of sodium hydroxide do you need: A) 50.0 g C) 40.0 g B) 20.0 g D) 80.0 g 35) 83.0 g of solid potassium iodide is dissolved in 250 mL of water. What is the molarity of the solution? A) 0.5 M C) 2.0 M B) 1.0 M D) 4.0 M 36) What is the molarity of a NaOH solution if there is 250 mL and 2.0 grams of NaOH? A) 0.20 M C) 0.40 M B) 0.30 M D) 0.60 M EQUILIBRIUM 37) When a reaction is at equilibrium and more reactant is added, which of the following changes is the immediate result? A) The reverse reaction rate remains the same. B) The forward reaction rate increases. C) The reverse reaction rate decreases. D) The forward reaction rate remains the same. Consider the following system at equilibrium… 2SO2 (g) + O2 (g) + heat 2 SO3 (g) 38) Which direction will the reaction shift if the heat is increased? A) Left B) Right C) No change 39) Which direction will the reaction shift if the pressure is decreased? A) Left B) Right C) No change 40) Which direction will the reaction shift if O2 is increased? A) Left B) Right C) No change 41) Which direction will the reaction shift if SO2 is increased? A) Left B) Right C) No change 42) Which direction will the reaction shift if there is an increase in pressure? A) Left B) Right C) No change ACIDS/BASES 43) Choose the pH of the solution that is most basic. A) 11 B) 12.7 C) 6.5 D) 4.0 44) Which of the following represents a conjugate acid-base pair? A) SO32- and SO2 C) H3O+ and H2 B) CO32- and CO2 D) NH4+ and NH3 45) The pH of a solution is 9. What is its H+ concentration? A) 1.0 x 10-9M C) 1.0 x 10-5 M B) 1.0 x 10-7M D) 9 M A chemistry student tests the pH of four different solutions. The results are in the table. Solution pH Lemon Juice 2.5 Milk 6.5 Sea Water 8.5 Ammonia 10.5 46) Which solution is weakly acidic? A) lemon juice C) seawater B) milk D) ammonia 47) What value of pH corresponds to a strongly basic solution? A) pH = 11 C) pH = 4 B) pH = 0 D) pH = 14 48) Strong acids _______________ A) Fully dissociate. C) precipitate in solution B) Partially dissociate D) Are insoluble 49) Ethanoic acid is a weak acid. Which one of the following particulate diagrams best represents ethanoic acid in solution in water? A) C) B) D) 50) What is the conjugate acid of HSO4-? A) H2SO4 C) H2O B) SO42- D) H3O+