Page 1. Name:

Size: px

Start display at page:

Download "Page 1. Name:"

Merryl Sherman
5 years ago
Views:

1 Name: 1) At 1 atmosphere and 298 K, 1 mole of H 2 O(l) molecules and 1 mole of C 2 H 5 OH(l) molecules both have the same A) mass B) density C) average kinetic energy D) vapor pressure 2) Two samples of gold that have different temperatures are placed in contact with one another. Heat will flow spontaneously from a sample of gold at 60DC to a sample of gold that has a temperature of A) 50DC B) 60DC C) 70DC D) 80DC 3) Which kelvin temperature is equivalent to -24DC? A) 273 K B) 226 K C) 297 K D) 249 K Page 1 4) At equilibrium, nitrogen, hydrogen, and ammonia gases form a mixture in a sealed container. The data table below gives some characteristics of these substances. Describe how to separate ammonia from hydrogen and nitrogen. 5) In which equation does the term "heat" represent heat of fusion? A) NaOH(aq) + HCl(aq) NaCl(aq) + H 2 O(l) + heat B) H 2 O(l) + heat H 2 O(g) C) NaCl(s) + heat NaCl(l) D) H 2 O(l) + HCl(g) H 3 O + (aq) + Cl - (aq) + heat 6) Given the particle diagram: At kpa and 298 K, which element could this diagram represent? A) Kr B) Ag C) Xe D) Rn 7) Which grouping of the three phases of bromine is listed in order from left to right for increasing distance between bromine molecules? A) solid, liquid, gas B) liquid, solid, gas C) solid, gas, liquid D) gas, liquid, solid 8) As the pressure on the surface of a liquid decreases, the temperature at which the liquid will boil A) remains the same C) increases B) decreases 9) Based on the Vapor Pressure of Four Liquids chemistry reference table, which substance has the weakest intermolecular forces? A) water B) propanone C) ethanol D) ethanoic acid 10) Using your knowledge of chemistry and the information in the Vapor Pressure of Four Liquids chemistry reference table, which statement concerning propanone and water at 50DC is true? A) Propanone has a lower vapor pressure and weaker intermolecular forces than water. B) Propanone has a lower vapor pressure and stronger intermolecular forces than water. C) Propanone has a higher vapor pressure and weaker intermolecular forces than water. D) Propanone has a higher vapor pressure and stronger intermolecular forces than water. 11) Which phase change results in the release of energy? A) H 2 O(g) H 2 O(l) C) H 2 O(l) H 2 O(g) B) H 2 O(s) H 2 O(l) D) H 2 O(s) H 2 O(g)

2 12) The graph below represents the uniform heating of a substance, starting below its melting point, when the substance is solid. Which line segments represent an increase in average kinetic energy? A) DE and EF B) AB and BC C) AB and CD D) BC and DE 13) Explain, in terms of molecular energy, why the vapor pressure of propanone increases when its temperature increases. 14) Given the graph below that represents the uniform cooling of a sample of lauric acid starting as a liquid above freezing point. 15) Under which conditions of temperature and pressure would helium behave most like an ideal gas? A) 750 K and 600 kpa B) 50 K and 600 kpa C) 50 K and 20 kpa D) 750 K and 20 kpa 16) The temperature of a 2.0-liter sample of helium gas at STP is increased to 27DC and the pressure is decreased to 80. kpa. What is the new volume of the helium sample? A) 2.0 L B) 1.4 L C) 2.8 L D) 4.0 L 17) At STP, 4 liters of O 2 contains the same total number of molecules as A) 4 L of CO 2 C) 2 L of Cl 2 B) 1 L of NH 3 D) 8 L of He Questions 18 and 19 refer to the following: Page 2 The diagram below shows a piston confining a gas in a cylinder. 18) Using the set of axes below, sketch the general relationship between the pressure and the volume of an ideal gas at constant temperature. 19) The gas volume in the cylinder is 6.2 milliliters and its pressure is 1.4 atmospheres. The piston is then pushed in until the gas volume is 3.1 milliliters while the temperature remains constant. Calculate the pressure, in atmospheres, after the change in volume. [Show all work.] (a) (b) (c) (d) Which line segment represents a phase change, only? What is the melting point of lauric acid? At which point do the particles of lauric acid have the highest average kinetic energy? Name the phase change that takes place during this 10-minute cooling time.

3 Questions 20 and 21 refer to the following: Cylinder A contains 22.0 grams of CO 2 (g) and cylinder B contains N 2 (g). The volumes, pressures, and temperatures of the two gases are indicated under each cylinder. 20) Explain why the number of molecules of N 2 (g) in cylinder B is the same as the number of molecules of CO 2 (g) in cylinder A. 21) The temperature of the CO 2 (g) is increased to 450. K and the volume of cylinder A remains constant. Show a correct numerical setup for calculating the new pressure of the CO 2 (g) in cylinder A. 22) What is the total number of oxygen atoms in the formula MgSO 4 d7h 2 O? [The d represents seven units of H 2 O attached to one unit of MgSO 4.] A) 11 B) 4 C) 5 D) 7 23) Which of these phrases best describes an atom? A) a hard sphere with negative particles uniformly embedded B) a hard sphere with positive particles uniformly embedded C) a positive nucleus surrounded by a hard negative shell D) a positive nucleus surrounded by a cloud of negative charges 24) The region that is the most probable location of an electron in an atom is A) the excited state B) an orbital C) an ion D) the nucleus 25) Which Lewis electron-dot diagram represents a boron atom in the ground state? A) C) B) D) Page 3 26) Which electron transition represents a gain of energy? A) from 3rd to 2nd shell B) from 2nd to 3rd shell C) from 3rd to 1st shell D) from 2nd to 1st shell 27) What determines the order of placement of the elements on the modern Periodic Table? A) the number of neutrons, only B) the number of neutrons and protons C) atomic number D) atomic mass 28) Which set of symbols represents atoms with valence electrons in the same electron shell? A) Ba, Br, Bi B) Mn, Hg, Cu C) Sr, Sn, I D) O, S, Te 29) An unknown element X can form a compound with the formula XBr 3. In which group on the Periodic Table would element X be found? A) 13 B) 1 C) 2 D) 14 30) As the elements in Period 2 of the Periodic Table are considered in succession from left to right, there is a decrease in atomic radius with increasing atomic number. This may best be explained by the fact that the A) number of protons increases, and the number of shells of electrons increases B) number of protons increases, and the number of shells of electrons remains the same C) number of protons decreases, and the number of shells of electrons increases D) number of protons decreases, and the number of shells of electrons remains the same 31) When an atom of phosphorus becomes a phosphide ion (P 3- ), the radius A) decreases C) remains the same B) increases 32) The high electrical conductivity of metals is primarily due to A) filled energy levels B) mobile electrons C) high ionization energies D) high electronegativities 33) Which change occurs when a barium atom loses two electrons? A) It becomes a negative ion and its radius increases. B) It becomes a negative ion and its radius decreases. C) It becomes a positive ion and its radius decreases. D) It becomes a positive ion and its radius increases. 34) At standard pressure, which element has a melting point higher than standard temperature? A) Br 2 B) Hg C) F 2 D) Fe

4 35) Which trends are observed when the elements in Period 3 on the Periodic Table are considered in order of increasing atomic number? A) The atomic radius decreases, and the first ionization energy generally increases. B) The atomic radius increases, and the first ionization energy generally increases. C) The atomic radius decreases, and the first ionization energy generally decreases. D) The atomic radius increases, and the first ionization energy generally decreases. 36) Based on the Properties of Selected Elements chemistry reference table, which of the following atoms requires the least energy for the removal of the most loosely bound electron? A) Br B) Sr C) Be D) Sn 37) Which list consists of elements that have the most similar chemical properties? A) K, Al, and Ni B) K, Ca, and Ga C) Mg, Al, and Si D) Mg, Ca, and Ba 38) At 298 K, oxygen (O 2 ) and ozone (O 3 ) have different properties because their A) atoms have different atomic numbers B) atoms have different atomic masses C) molecules have different average kinetic energies D) molecules have different molecular structures 39) Which statement correctly describes diamond and graphite, which are different forms of solid carbon? A) They do not differ in their molecular structure or properties. B) They differ in their properties, only. C) They differ in their molecular structure and properties. D) They differ in their molecular structure, only. 40) Potassium ions are essential to human health. The movement of dissolved potassium ions, K + (aq), in and out of a nerve cell allows that cell to transmit an electrical impulse. What property of potassium ions allows them to transmit an electrical impulse in the situation described? Questions 41 and 42 refer to the following: The table below shows the electronegativity of selected elements of Period 2 of the Periodic Table. 41) (a) On the grid below, set up a scale for electronegativity on the y-axis. (b) (c) Plot the data by drawing a best-fit line. Using the graph, predict the electronegativity of nitrogen. 42) For the elements in the table, state the trend in electronegativity in terms of atomic number. 43) As two chlorine atoms combine to form a molecule, energy is A) released B) destroyed C) created D) absorbed 44) Which of the following elements has the least attraction for electrons in a chemical bond? A) chlorine B) fluorine C) nitrogen D) oxygen Page 4 45) Which of the following solids has the highest melting point? A) SO 2 (s) C) H 2 O(s) B) CO 2 (s) D) Na 2 O(s)

5 46) What is the correct Lewis electron-dot structure for the compound magnesium fluoride? A) Page 5 51) Which formula represents a nonpolar molecule? A) HCl C) H 2 O B) CF 4 D) NH 3 52) Which Lewis electron-dot diagram is correct for CO 2? B) A) C) C) B) D) D) 47) Which compound contains both ionic and covalent bonds? A) CaCO 3 C) PCl 3 B) CH 2 O D) MgF 2 48) A solid substance was tested in the laboratory. The test results are listed below. d dissolves in water d is an electrolyte d melts at a high temperature 53) Molecules in a sample of NH 3 (l) are held closely together by intermolecular forces A) caused by different numbers of neutrons B) existing between ions C) caused by unequal charge distribution D) existing between electrons 54) The table below shows the normal boiling point of four compounds. Based on these results, the solid substance could be A) C C) Cu B) CuBr 2 D) C 6 H 12 O 6 C) H 2 49) Which molecule contains a triple covalent bond? A) N 2 B) Cl 2 D) O 2 50) Which substance is correctly paired with its type of bonding? A) NaBr nonpolar covalent B) HCl nonpolar covalent C) Br 2 polar covalent D) NH 3 polar covalent Which compound has the strongest intermolecular forces? A) HCl(l) B) CH 3 F(l) C) HF(l) D) CH 3 Cl(l)

6 55) In the boxes below, draw a correct Lewis electron-dot structure for: Page 6 (a) an atom of hydrogen (b) an atom of nitrogen (c) a molecule of ammonia (NH 3 ) Questions 56 and 57 refer to the following: Naphthalene, a nonpolar substance that sublimes at room temperature, can be used to protect wool clothing from being eaten by moths. 56) Explain, in terms of intermolecular forces, why naphthalene sublimes. 57) Explain why naphthalene is not expected to dissolve in water. 58) The solubility of KClO 3 (s) in water increases as the A) temperature of the solution increases B) temperature of the solution decreases C) pressure on the solution increases D) pressure on the solution decreases 59) At room temperature, the solubility of which solute in water would be most affected by a change in pressure? A) carbon dioxide B) methanol C) sodium nitrate D) sugar 60) What is the molarity of a solution of NaOH if 2 liters of the solution contains 4 moles of NaOH? A) 80 M B) 0.5 M C) 2 M D) 8 M 61) What is the concentration of a solution, in parts per million, if 0.02 gram of Na 3 PO 4 is dissolved in 1,000 grams of water? A) 20 ppm B) 0.2 ppm C) 0.02 ppm D) 2 ppm 62) What occurs when NaCl(s) is added to water? A) The boiling point of the solution increases, and the freezing point of the solution increases. B) The boiling point of the solution increases, and the freezing point of the solution decreases. C) The boiling point of the solution decreases, and the freezing point of the solution decreases. D) The boiling point of the solution decreases, and the freezing point of the solution increases. 63) Based on the Solubility Curves chemistry reference table, what is the maximum number of grams of KCl(s) that will dissolve in 200 grams of water at 50DC to produce a saturated solution? A) 42 g B) 58 g C) 84 g D) 38 g 64) According to Solubility Curves chemistry reference table, which solution is saturated at 30DC? A) 30 grams of NaCl in 100 grams of water B) 12 grams of KClO 3 in 100 grams of water C) 30 grams of NaCl in 200 grams of water D) 12 grams of KClO 3 in 200 grams of water 65) A student is instructed to make liter of a M aqueous solution of Ca(NO 3 ) 2. Show a correct numerical setup for calculating the total number of moles of Ca(NO 3 ) 2 needed to make liter of a M calcium nitrate solution. 66) Sulfur dioxide, SO 2, is one of the gases that react with water to produce acid rain. According to the Solubility Curves chemistry reference table, describe how the solubility of sulfur dioxide in water is affected by an increase in water temperature.

7 Questions 67 and 68 refer to the following: A student uses 200 grams of water at a temperature of 60DC to prepare a saturated solution of potassium chloride, KCl. 67) The solution described is cooled to 10DC and the excess KCl precipitates (settles out). The resulting solution is saturated at 10DC. How many grams of KCl precipitated out of the original solution? 68) According to the Solubility Curves chemistry reference table, how many grams of KCl must be used to create the saturated solution described? Questions 69 through 71 refer to the following: FIZZIES - A SPLASH FROM THE PAST They're baaack... a splash from the past! Fizzies instant sparkling drink tablets, popular in the 1950's and 1960's, are now back on the market. What sets them apart from other powdered drinks is that they bubble and fizz when placed in water, forming an instant carbonated beverage. The fizz in Fizzies is caused by bubbles of carbon dioxide (CO 2 ) gas that are released when the tablet is dropped into water. Careful observation reveals that these bubbles rise to the surface because CO 2 gas is much less dense than water. However, not all of the CO 2 gas rises to the surface; some of it dissolves in the water. The dissolved CO 2 can react with water to form carbonic acid, H 2 CO 3. H 2 O(l) + CO 2 (aq) Š H 2 CO 3 (aq) 71) (a) Describe the solubility of CO 2 gas in water. (b) Explain your response to part (a) in terms of the molecular polarities of CO 2 (g) and H 2 O(l). 72) Given the balanced equation: 4Fe(s) + 3O 2 (g) 2Fe 2 O 3 (s) + 1,640 kj Which phrase best describes this reaction? A) endothermic with DH = -1,640 kj B) endothermic with DH = +1,640 kj C) exothermic with DH = +1,640 kj D) exothermic with DH = -1,640 kj 73) When a spark is applied to a mixture of hydrogen and oxygen, the gases react explosively. Which potential energy diagram best represents the reaction? A) B) Page 7 The ph of the Fizzies drink registers between 5 and 6, showing that the resulting solution is clearly acidic. Carbonic acid is found in other carbonated beverages as well. One of the ingredients on any soft drink label is carbonated water, which is another name for carbonic acid. However, in the production of soft drinks, the CO 2 is pumped into the solution under high pressure at the bottling plant. Brian Rohrig, Excerpted from "Fizzies A Splash from the Past," Chem Matters, February ) What is the only positive ion in an aqueous solution of carbonic acid? 70) CO 2 is pumped into the soft drink solution under high pressure. Why is high pressure necessary? C) D)

8 74) The potential energy diagram below represents a reaction Page 8 75) Given the potential energy diagram for a chemical reaction: Which arrow represents the activation energy of the forward reaction? A) A B) B C) C D) D Which statement correctly describes the energy changes that occur in the forward reaction? A) The activation energy is 10. kj and the reaction is exothermic. B) The activation energy is 50. kj and the reaction is endothermic. C) The activation energy is 10. kj and the reaction is endothermic. D) The activation energy is 50. kj and the reaction is exothermic. 76) In each of the four beakers shown below, a 2.0-centimeter strip of magnesium ribbon reacts with 100 milliliters of HCl(aq) under the conditions shown. In which beaker will the reaction occur at the fastest rate? A) A B) B C) C D) D 77) Which statement best explains the role of a catalyst in a chemical reaction? A) A catalyst is added as an additional reactant and is consumed but not regenerated. B) A catalyst limits the amount of reactants used. C) A catalyst changes the kinds of products produced. D) A catalyst provides an alternate reaction pathway that requires less activation energy. 78) A catalyst is added to a system at equilibrium. If the temperature remains constant, the activation energy of the forward reaction A) remains the same C) decreases B) increases 79) Which sample has the lowest entropy? A) 1 mole of KNO 3 (s) C) 1 mole of H 2 O(l) B) 1 mole of H 2 O(g) D) 1 mole of KNO 3 (l)

9 80) Systems in nature tend to undergo changes toward A) higher energy and higher entropy B) lower energy and lower entropy C) higher energy and lower entropy D) lower energy and higher entropy 81) In the smelting of iron ore, Fe 2 O 3 is reduced in a blast furnace at high temperature by a reaction with carbon monoxide. Crushed limestone, CaCO 3, is also added to the mixture to remove impurities in the ore. The carbon monoxide is formed by the oxidation of carbon (coke), as shown in the following reaction: 2C + O 2 2CO + energy Liquid iron flows from the bottom of the blast furnace and is processed into different alloys of iron. Using the set of axes provided, sketch a potential energy diagram for the reaction of carbon and oxygen that produces the carbon monoxide in the situation described. 84) Given the equilibrium reaction at STP: N 2 O 4 (g) Š 2NO 2 (g) Page 9 Which statement correctly describes this system? A) The concentrations of N 2 O 4 and NO 2 are both increasing. B) The forward and reverse reaction rates are equal. C) The forward and reverse reaction rates are both increasing. D) The concentrations of N 2 O 4 and NO 2 are equal. 85) A student adds solid KCl to water in a flask. The flask is sealed with a stopper and thoroughly shaken until no more solid KCl dissolves. Some solid KCl is still visible in the flask. The solution in the flask is A) unsaturated and is not at equilibrium with the solid KCl B) saturated and is not at equilibrium with the solid KCl C) saturated and is at equilibrium with the solid KCl D) unsaturated and is at equilibrium with the solid KCl 86) Given the reaction at equilibrium: A(g) + B(g) Š AB(g) + heat 82) Which statement correctly describes a chemical reaction at equilibrium? A) The concentrations of the products and reactants are equal. B) The concentrations of the products and reactants are constant. C) The rate of the forward reaction is greater than the rate of the reverse reaction. D) The rate of the forward reaction is less than the rate of the reverse reaction. 83) Which statement about a system at equilibrium is true? A) The forward reaction rate is less than the reverse reaction rate. B) The forward reaction rate stops and the reverse reaction rate continues. C) The forward reaction rate is greater than the reverse reaction rate. D) The forward reaction rate is equal to the reverse reaction rate. The concentration of A(g) can be increased by A) increasing the concentration of B(g) B) adding a catalyst C) lowering the temperature D) increasing the concentration of AB(g) 87) Which species can conduct an electric current? A) CH 3 OH(aq) C) NaOH(s) B) HCl(aq) D) H 2 O(s) 88) The only positive ion found in an aqueous solution of sulfuric acid is the A) sulfate ion B) hydronium ion C) sulfite ion D) hydroxide ion 89) Which substance is an Arrhenius acid? A) Mg(OH) 2 (aq) C) HBr(aq) B) CH 3 CHO D) LiF(aq) 90) How are HNO 3 (aq) and CH 3 COOH(aq) similar? A) They are Arrhenius acids and they turn blue litmus red. B) They are Arrhenius bases and they turn blue litmus red. C) They are Arrhenius acids and they turn red litmus blue. D) They are Arrhenius bases and they turn red litmus blue. 91) One acid-base theory states that an acid is A) an electron donor C) an OH - donor B) a neutron donor D) an H + donor 92) Which of these ph numbers indicates the highest level of acidity? A) 12 B) 5 C) 10 D) 8

10 Page 10 93) Which of these 1 M solutions will have the highest ph? A) NaCl C) CH 3 OH B) HCl D) NaOH 94) When the ph of a solution changes from a ph of 5 to a ph of 3, the hydronium ion concentration is A) 100 times the original content B) 10 times the original content C) 0.01 of the original content D) 0.1 of the original content 95) Which indicator is yellow in a solution with a ph of 9.8? A) methyl orange B) thymol blue C) bromthymol blue D) bromcresol green 96) A student was given four unknown solutions. Each solution was checked for conductivity and tested with phenolphthalein. The results are shown in the data table below. 97) Which equation represents a neutralization reaction? A) Ni(NO 3 ) 2 + H 2 S NiS + 2HNO 3 B) NaCl + AgNO 3 AgCl + NaNO 3 C) H 2 SO 4 + Mg(OH) 2 MgSO 4 + 2H 2 O D) Na 2 CO 3 + CaCl 2 2NaCl + CaCO 3 98) Sulfuric acid, H 2 SO 4 (aq), can be used to neutralize barium hydroxide, Ba(OH) 2 (aq). What is the formula for the salt produced by this neutralization? A) BaSO 3 C) BaS B) BaSO 2 D) BaSO 4 99) What is the molarity of an HCl solution if 20. milliliters of this acid is needed to neutralize 10. milliliters of a 0.50 M NaOH solution? A) 1.0 M B) 0.50 M C) 0.25 M D) 0.75 M Based on the data table, which unknown solution could be 0.1 M NaOH? A) A B) B C) C D) D 100) Four flasks each contain 100 milliliters of aqueous solutions of equal concentrations at 25DC and 1 atm. (a) (b) (c) (d) (e) Which solutions contain electrolytes? Which solution has the lowest ph? What causes some aqueous solutions to have a low ph? Which solution is most likely to react with an Arrhenius acid to form a salt and water? Which solution has the lowest freezing point? [Explain your answer.]

(g) burns according to this reaction? D) CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(l)

(g) burns according to this reaction? D) CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(l) Name: 7171-1 - Page 1 1) In a chemical reaction, the difference between the potential energy of the products and the potential energy of the reactants is defined as the A) heat of reaction B) ionization