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CHEM 1305. Review for Test 2 (chapter 7-12). Central. S118 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The compound NH3 is classified as which of the following? 1) _______ A) binary ionic B) ternary ionic C) binary molecular D) binary acid E) ternary oxyacid 2) What is the Stock system name for Cu2+? A) cupric ion B) copper ion C) copper(II) ion D) cuprous ion E) cuprum ion 2) _______ 3) What is the systematic name for S2-? 3) _______ A) sulfur ion B) sulfite ion C) sulfide ion D) sulfate ion E) none of the above 4) What is the systematic name for CrO42-? 4) _______ A) chromide ion B) dichromate ion C) chromate ion D) chromite ion E) none of the above 5) What is the chemical formula for the acetate ion? A) C2H3O2- 5) _______ B) HCO32C) HCO3D) C2H3O22E) none of the above 6) What is the chemical formula for the binary compound of Au 3+ and I- ions? A) AuI3 B) AuI C) Au3I3 D) Au3I E) none of the above 7) What is the ionic charge for the lead ion in PbS 2? 7) _______ A) 2+ B) zero C) 1+ D) 4+ pg. 1 CHEM 1305. Review for Test 2 (chapter 7-12). Central. S118 6) _______ E) none of the above 8) What is the chemical formula for the binary compound of Co 3+ and O2- ions? 8) _______ A) CoO B) Co3O2 C) Co2O3 D) Co6O6 E) none of the above 9) What is the chemical formula for lithium fluoride? A) LiF B) LiF3 9) _______ C) LiF2 D) Li3F2 E) none of the above 10) What is the ionic charge for the chromium ion in Cr2(SO4)3? 10) ______ A) 1+ B) 2+ C) 3+ D) 4+ E) none of the above 11) What is the chemical formula for the ferrous ion? A) Fe3+ 11) ______ B) F2+ C) Fe2+ D) F3+ E) none of the above 12) What is the chemical formula for iodine heptafluoride? A) IF6 12) ______ B) IF7 C) IF D) I2F6 E) none of the above 13) What is the systematic name for aqueous HF? A) fluoric acid B) hydrogen fluoride C) fluorous acid D) hydrofluoric acid E) none of the above 13) ______ 14) What is the chemical formula for chlorous acid? A) HClO(aq) B) HClO3(aq) 14) ______ C) HClO2(aq) D) HClO4(aq) pg. 2 CHEM 1305. Review for Test 2 (chapter 7-12). Central. S118 E) none of the above 15) Which of the following changes is evidence of a chemical reaction? A) A change in color is observed. B) A change in volume is observed. C) A change in physical state is observed. D) all of the above E) none of the above 15) ______ 16) Which of the following symbolizes a substance dissolved in water? A) (s) B) (l) C) (g) D) (aq) E) none of the above 16) ______ 17) What is the coefficient of oxygen gas after balancing the following equation? __P(s) + __O2(g) → __P2O3(s) 17) ______ A) 1 B) 2 C) 5 D) 3 E) none of the above 18) What is the coefficient of CO2 gas after balancing the following equation? __KHCO3(s) __K2CO3(s) + __H2O(g) + __CO2(g) 18) ______ A) 1 B) 2 C) 3 D) 4 E) none of the above 19) What type of chemical reaction is illustrated in the following example? Zn(s) + HCl(aq) → ZnCl2(aq) + H2(g) 19) ______ A) combination reaction B) decomposition reaction C) single-replacement reaction D) double-replacement reaction E) neutralization reaction 20) What is the predicted product from the following combination reaction? K(s) + Cl2(g) 20) ______ pg. 3 CHEM 1305. Review for Test 2 (chapter 7-12). Central. S118 A) KCl2B) KCl3 C) K3Cl D) K2ClE) KCl 21) What are the predicted products from the following decomposition reaction? Ca(HCO3)2(s) 21) ______ A) Ca, H2O, and CO2 B) CaCO3 and H2O C) CaCO3, H2O, and CO2 D) Ca, H2, and CO2 E) CaCO3, H2, and CO2 22) Which of the following metals reacts with aqueous Mg(NO3)2? Partial Activity Series: Mg > Al > Zn > (H) > Cu 22) ______ A) Cu B) Zn C) Al D) all of the above E) none of the above 23) What are the products from the following single-replacement reaction? Mg(s) + HNO3(aq) → 23) ______ A) Mg(NO3)2 and H2O B) Mg(NO2)2 and H2 C) Mg(NO2)2 and H2O D) Mg(NO3)2 and H2 E) no reaction 24) Which of the following compounds is soluble in water? A) NiCO3 24) ______ B) ZnCO3 C) (NH4)2CO3 D) all of the above E) none of the above 25) What are the products from the following double-replacement reaction? AgNO3(aq) + K2CrO4(aq) → 25) ______ A) Ag2CrO3 and KNO3 B) Ag2CrO4 and KNO2 C) Ag2CrO4 and KNO3 D) Ag2CrO3 and KNO2 E) no reaction pg. 4 CHEM 1305. Review for Test 2 (chapter 7-12). Central. S118 26) What are the products from the following neutralization reaction? HC2H3O2(aq) + Ca(OH)2(aq) → 26) ______ A) Ca(HCO3)2 and H2O B) Ca(C2H3O2)2 and H2O C) Ca(C2H3O2)2 and H2 D) Ca(HCO3)2 and H2 E) no reaction 27) How many Co atoms equal a mass of 58.93 g? (Refer to the Periodic Table.) A) 1 B) 6.02 × 1023 27) ______ C) 27 D) 59 E) none of the above 28) How many atoms of copper are in 2.50 mol Cu metal? A) 1.51 × 1023 atoms 28) ______ B) 1.51 × 1024 atoms C) 2.41 × 1023 atoms D) 1.5l × 1022 atoms E) 2.41 × 1024 atoms 29) What is the molar mass of cholesterol, C27H45OH? 29) ______ A) 386.73 g/mol B) 432.79 g/mol C) 30.03 g/mol D) 448.79 g/mol E) 431.78 g/mol 30) What is the mass of 3.30 × 1023 atoms of silver, Ag? 30) ______ A) 59.1 g B) 85.7 g C) 25.8 g D) 0.549 g E) 197 g 31) How many ethane molecules are in 22.4 liters of C2H6 gas at STP? 31) ______ A) 6.02 × 1023 molecules B) 1.20 × 1024 molecules C) 2.69 × 1022 molecules D) 1.35 × 1025 molecules E) 1.81 × 1024 molecules 32) What is the volume of 2.75 × 1024 molecules of nitrogen dioxide gas, NO2, at STP? A) 0.204 L B) 102 L C) 4.90 L D) 4.57 L 32) ______ E) 0.00977 L 33) The formula for mustard gas used in chemical warfare is C 4H8SCl2 (159.09 g/mol). What is the percentage of carbon in the compound? 33) ______ A) 7.55% B) 20.16% C) 5.08% D) 30.20% E) 44.57% pg. 5 CHEM 1305. Review for Test 2 (chapter 7-12). Central. S118 34) If 0.225 mol of tin combines with 0.450 mol of sulfur, what is the empirical formula of the tin sulfide product? 34) ______ A) Sn3S3 B) SnS C) Sn2S D) SnS2 E) none of the above 35) The taste of sour milk is lactic acid. What is the molecular formula for lactic acid if the percent composition is 40.00% C, 6.71% H, 53.29% O, and the approximate molar mass is 90 g/mol? 35) ______ A) C3H6O3 B) C6HO8 C) CH2O D) CHO2 E) CHO 36) The insulating and packing material Styrofoam is a polymer of styrene. Find the molecular formula of styrene given its percent composition: 92.25% C, 7.75% H. The approximate molar mass of styrene is 104 g/mol. 36) ______ A) C12H B) CH12 C) C8H8 D) CH8 E) CH 37) Fructose is a sugar found in fruit and honey. Calculate the empirical formula for fructose given its percent composition: 40.00% C, 6.72% H, and 53.29% O. 37) ______ A) CHO2 B) C6HO8 C) CH2O D) CHO E) C3H6O3 38) An emerald gemstone is an impure form of the mineral beryl, Be3Al2Si16O18 (818.43 g/mol). What is the percentage of aluminum in the mineral? A) 35.2% 38) ______ B) 54.9% C) 3.30% D) 3.37% E) 6.59% 39) If 1.00 L of an unknown gas at STP has a mass of 5.40 g, what is its molar mass? A) 4.15 g/mol B) 54.0 g/mol C) 22.4 g/mol D) 121 g/mol E) 5.40 g/mol 39) ______ 40) How many moles NO2 gas are produced from the reaction of 1 mole O2 gas according to the balanced chemical equation? 2 NO(g) + O2(g) 2 NO2(g) 40) ______ A) 1 mol NO2 B) 2 mol NO2 C) 4 mol NO2 D) 0.5 mol NO2 E) none of the above 41) How many moles of hydrogen gas react to yield 1.00 mol of hydrogen iodide? __H2(g) + __ I2 (g) __HI(g) 41) ______ pg. 6 CHEM 1305. Review for Test 2 (chapter 7-12). Central. S118 A) 2.00 mol H2 B) 4.00 mol H2 C) 1.00 mol H2 D) 0.500 mol H2 E) none of the above 42) Classify the following type of stoichiometry problem: How many grams of tin must react with an excess volume of nitric acid to produce 50.0 mL of hydrogen gas? 42) ______ A) mass mass problem B) mass volume problem C) volume volume problem D) mole mole problem E) none of the above 43) What is the mass of insoluble silver bromide (187.77 g/mol) produced from 2.96 g of iron(III) bromide (295.55 g/mol) and aqueous silver nitrate? __FeBr3(s) + __AgNO3(aq) → __AgBr(s) + __Fe(NO3)3(aq) 43) ______ A) 3.76 g AgBr B) 0.627 g AgBr C) 0.940 g AgBr D) 1.88 g AgBr E) 5.64 g AgBr 44) What is the volume of oxygen gas at STP from the decomposition of 1.70 g of sodium nitrate (85.00 g/mol)? __NaNO3(s) __NaNO2(s) + __O2(g) A) 0.448 L O2 B) 0.896 L O2 C) 12.9 L O2 44) ______ D) 3.23 L O2 E) 0.224 L O2 45) What volume of hydrogen gas reacts to produce 12.0 mL of ammonia gas? (Assume temperature and pressure remain constant.) __N2(g) + __H2(g) __NH3(g) 45) ______ A) 4.00 mL H2 B) 36.0 mL H2 C) 18.0 mL H2 D) 6.00 mL H2 E) none of the above 46) Considering the limiting reactant concept, how many moles of C are produced from the reaction of 2.00 mol A and 4.50 mol B? A(g) + 2 B(g) → 3 C(g) 46) ______ A) 2.00 mol C B) 6.75 mol C pg. 7 CHEM 1305. Review for Test 2 (chapter 7-12). Central. S118 C) 4.50 mol C D) 6.00 mol C E) none of the above 47) Considering the limiting reactant, what is the mass of iron produced from 75.0 g of iron(II) oxide (71.85 g/mol) and 25.0 g of magnesium metal? FeO(l) + Mg(l) A) 58.3 g Fe B) 28.7 g Fe Fe(l) + MgO(s) C) 57.4 g Fe 47) ______ D) 100.0 g Fe E) 29.1 g Fe 48) Starting with 1.56 g of salicylic acid, a student prepares 1.75 g of aspirin. If the calculated mass of aspirin is 1.88 g, what is the percent yield? 48) ______ A) 93.1% B) 83.0% C) 107% D) 121% E) 89.1% 49) The decomposition of 1.500 g of potassium chlorate evolved 405 mL of oxygen gas. If the calculated volume of oxygen gas is 411 mL, what is the percent yield? 49) ______ A) 148% B) 67.3% C) 101% D) 65.7% E) 98.5% 50) Considering the limiting reactant, what is the volume of NO gas produced from 50.0 L of ammonia gas and 60.0 L of oxygen gas? (Assume constant conditions.) 4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(g) 50) ______ A) 75.0 L NO B) 110.0 L NO C) 50.0 L NO D) 48.0 L NO E) 60.0 L NO 51) Considering the limiting reactant concept, how many moles of cobalt(III) oxide are produced from the reaction of 1.00 mol of cobalt and 1.00 mol of oxygen gas? 4 Co(s) + 3 O2(g) 2 Co2O3(s) 51) ______ A) 0.500 mol Co2O3 B) 2.00 mol Co2O3 C) 0.667 mol Co2O3 D) 1.50 mol Co2O3 E) none of the above 52) What volume of methane gas, CH4, reacts to give 5.00 mL of carbon dioxide gas? (Assume temperature and pressure remain constant.) __CH4(g) + __O2(g) __CO2(g) + __H2O(g) 52) ______ pg. 8 CHEM 1305. Review for Test 2 (chapter 7-12). Central. S118 A) 5.00 mL CH4 B) 20.0 mL CH4 C) 10.0 mL CH4 D) 2.50 mL CH4 E) none of the above 53) The N3- ion is classified as which of the following? A) monoatomic cation B) monoatomic anion C) polyatomic cation D) polyatomic anion E) none of the above 53) ______ 54) What is the predicted ionic charge for a metal in Group IIIA/13? A) 5B) 3+ C) 5+ D) 3E) none of the above 54) ______ 55) What is the chemical formula for barium phosphate? 55) ______ A) BaPO4 B) Ba2(PO4)3 C) BaPO3 D) Ba3(PO4)2 E) none of the above 56) What is the coefficient of water after balancing the following equation? __HC2H3O2(aq) + __Ca(OH)2(aq) → __Ca(C2H3O2)2(aq) + __H2O(l) A) 1 B) 2 C) 3 D) 6 E) none of the above 57) What type of chemical reaction is illustrated in the following example? HNO3(aq) + KOH(aq) → KNO3(aq) + H2O(l) 57) ______ A) combination reaction B) decomposition reaction C) single-replacement reaction D) double-replacement reaction E) neutralization reaction 58) What are the products from the following single-replacement reaction? Ca(s) + H2O(l) → 58) ______ pg. 9 CHEM 1305. Review for Test 2 (chapter 7-12). Central. S118 56) ______ A) CaO and H2 B) Ca(OH)2 and H2 C) Ca(OH)2 and H2O D) CaO and H2O E) no reaction 59) What is the mass of 0.455 L of ethane gas, C2H6, at STP? A) 0.611 g B) 2.95 g C) 10.2 g D) 0.340 g 59) ______ E) 65.9 g 60) The formula for mustard gas used in chemical warfare is C 4H8SCl2 (159.09 g/mol). What is the percentage of chlorine in the compound? A) 44.57% 60) ______ B) 20.16% C) 30.20% D) 22.28% E) 5.08% 61) If 1.888 g of bismuth metal reacts with sulfur to give 2.323 g of bismuth sulfide, what is the empirical formula of the product? 61) ______ A) BiS2 B) BiS C) BiS3 D) Bi3S2 E) Bi2S3 62) What is the mass of mercuric oxide (216.59 g/mol) that decomposes to release 0.750L of oxygen gas at STP? __HgO(s) __Hg(l) + __O2(g) 62) ______ A) 3.63 g HgO B) 14.5 g HgO C) 0.155 g HgO D) 0.0388 g HgO E) 7.25 g HgO 63) What volume of propane gas, C3H8, reacts to give 3.00 L of carbon dioxide gas? (Assume temperature and pressure remain constant.) __C3H8(g) + __O2(g) __CO2(g) + __H2O(g) 63) ______ A) 25.0 L C3H8 B) 1.00 L C3H8 C) 20.0 L C3H8 D) 15.0 L C3H8 E) none of the above 64) Considering the limiting reactant concept, how many moles of cobalt(II) oxide are produced from the reaction of 1.00 mol of cobalt and 1.00 mol of oxygen gas? 2 Co(s) + O2(g) 2 CoO(s) 64) ______ A) 1.50 mol CoO B) 2.00 mol CoO pg. 10 CHEM 1305. Review for Test 2 (chapter 7-12). Central. S118 C) 1.00 mol CoO D) 0.500 mol CoO E) none of the above 65) Considering the limiting reactant, what is the mass of manganese produced from 25.0 g of manganese(IV) oxide (86.94 g/mol) and 25.0 g of aluminum metal? 3 MnO2(l) + 4 Al(l) A) 15.8 g Mn B) 67.8 g Mn 3 Mn(l) + 2 Al2O3(s) C) 50.9 g Mn 65) ______ D) 38.2 g Mn E) 47.4 g Mn 66) The decomposition of 1.500 g of baking soda gave 0.200 L of carbon dioxide gas. If the calculated volume of carbon dioxide gas is 0.210 L, what is the percent yield? 66) ______ A) 63.5% B) 70.0% C) 105% D) 158% E) 95.2% 67) The decomposition of 1.500 g of sodium nitrate produced 195 mL of oxygen gas. If the calculated volume of oxygen gas is 198 mL, what is the percent yield? 67) ______ A) 68.0% B) 98.5% C) 102% D) 152% E) 65.7% 68) What is the mass of silver metal produced from 6.35 g of copper metal? __Cu(s) + __AgNO3(aq) → __Cu(NO3)2(aq) + __Ag(s) A) 0.187 g Ag B) 21.6 g Ag C) 1.08 g Ag D) 0.540 g Ag 68) ______ E) 0.747 g Ag 69) How many moles of hydrogen gas are produced from 0.500 mol of water? __Ca(s) + __H2O(l) → __Ca(OH)2(aq) + __H2(g) 69) ______ A) 0.500 mol H2 B) 2.00 mol H2 C) 0.250 mol H2 D) 1.00 mol H2 E) none of the above 70) Which of the following is an observed property of gases? A) gases have a high density B) gases have a fixed shape C) gases compress infinitely D) all of the above E) none of the above 70) ______ 71) Which of the following expresses standard atmospheric pressure? A) 76 cm Hg B) 1 atm C) 14.7 psi D) all of the above E) none of the above pg. 11 CHEM 1305. Review for Test 2 (chapter 7-12). Central. S118 71) ______ 72) If a barometer reads 535 mm Hg, what is the atmospheric pressure expressed in centimeters of mercury? ______ 72) A) 535 cm Hg B) 53,500 cm Hg C) 53.5 cm Hg D) 5.35 cm Hg E) 5350 cm Hg 73) An aluminum scuba tank contains compressed air at 2750 psi. What is the pressure expressed in atmospheres? 73) ______ A) 36.2 atm B) 187 atm C) 4.04 × 104 atm D) 3.62 atm E) 92.0 atm 74) Which of the following decreases the pressure of a gas? A) increasing the number of gas molecules B) increasing the temperature C) decreasing the volume D) all of the above E) none of the above 74) ______ 75) If a piston compresses air in a steel cylinder, what happens in the cylinder? A) the volume decreases, and the pressure increases B) the volume decreases, and the pressure decreases C) the volume increases, and the pressure decreases D) the volume increases, and the pressure increases E) none of the above 75) ______ 76) A sample of neon gas at 1.20 atm compresses from 0.250 L to 0.125 L. If the temperature remains constant, what is the final pressure in atm? 76) ______ A) 2.40 atm B) 1.00 atm C) 0.600 atm D) 1.20 atm E) none of the above 77) A sample of krypton gas at 75.0 psi expands from 0.100 L to 0.450 L. If the temperature remains constant, what is the final pressure in psi? 77) ______ A) 0.167 psi B) 16.7 psi C) 3.38 psi D) 338 psi E) 75.0 psi 78) If the pressure of 125 cm3 of nitrogen gas at 100°C decreases from 885 torr to 225 torr, what is the final volume? (Assume temperature remains constant.) 78) ______ A) 0.318 cm3 B) 492 cm3 C) 4.92 cm3 D) 4590 cm3 pg. 12 CHEM 1305. Review for Test 2 (chapter 7-12). Central. S118 E) 31.8 cm3 79) Which of the following graphs represents the volume versus Kelvin temperature for a gas at constant pressure? 79) ______ A) (a) B) (b) C) (c) D) (d) E) (e) 80) A 50.0 mL volume of propane gas is cooled from 60.0°C to 30.0°C. If the pressure remains constant, what is the final volume in milliliters? 80) ______ A) 50.0 mL B) 55.0 mL C) 100.0 mL D) 25.0 mL E) 45.5 mL 81) If a volume of oxygen gas at 45.0°C decreases from 50.0 mL to 25.0 mL, what is the final Celsius temperature? Assume pressure remains constant. 81) ______ A) 636°C B) -114°C C) 159°C D) 363°C E) 23°C 82) A sample of air at 7.50 atm is cooled from 448K to 224K. If the volume remains constant, what is the final pressure? 82) ______ A) 4.57 atm B) 3.75 atm C) 6.15 atm D) 12.3 atm E) 15.0 atm 83) A sample of helium gas has a temperature of 100 K. What is the final temperature if both the volume and pressure each double? 83) ______ A) 400 K B) 50 K C) 100 K D) 200 K 84) What is the vapor pressure of water at 100°C? A) 1 mm Hg B) 760 mm Hg C) 100 mm Hg D) 76 mm Hg E) none of the above E) 25 K 84) ______ 85) In a famous experiment, Stanley Miller provided evidence for the theory of evolution. He placed CH 4, NH3, H2, and H2O in a glass sphere and excited the gases using electricity and UV light. If the partial pressures of the gases were 340 mm Hg, 125 mm Hg, 65 mm Hg, and 100 mm Hg, what was the total pressure in the glass sphere? 85) ______ pg. 13 CHEM 1305. Review for Test 2 (chapter 7-12). Central. S118 A) 630 mmHg B) 340 mmHg C) 130 mmHg D) 760 mmHg E) none of the above 86) At the same temperature, which of the following gases contains molecules with the fastest average velocity? ______ 86) A) ozone, O3 B) hydrogen, H2 C) nitrogen, N2 D) oxygen, O2 E) The average velocity is the same. 87) If 1.06 mol of helium exert a pressure of 0.750 atm at 210.0°C, what is the volume in liters? (R = 0.0821 atm•L/mol•K) 87) ______ A) 24.4 L B) 4160 L C) 56.0 L D) 0.00155 L 88) Predict which of the following has an ionic bond. A) ICl B) HI C) IBr D) all of the above E) none of the above E) 28.1 L 88) ______ 89) Predict which of the following has a covalent bond. 89) ______ A) HF B) IBr C) BrCl D) all of the above E) none of the above 90) Which of the following statements is TRUE regarding an ionic bond? 90) ______ A) The ionic radius of a nonmetal ion is greater than its atomic radius. B) Breaking an ionic bond between two ions releases energy. C) Metal atoms gain electrons and nonmetal atoms lose electrons. D) all of the above E) none of the above 91) Which of the following statements is TRUE regarding a covalent bond? A) Breaking a covalent bond between two atoms releases energy. B) The bond length is less than the sum of the two atomic radii. C) Valence electrons are transferred between two nonmetal atoms. D) all of the above E) none of the above 91) ______ 92) What is the total number of valence electrons in one molecule of N 2H4? 92) ______ A) 18 B) 2 pg. 14 CHEM 1305. Review for Test 2 (chapter 7-12). Central. S118 C) 8 D) 14 E) none of the above 93) What is the total number of valence electrons in a hydronium ion, H 3O+? 93) ______ A) 9 B) 10 C) 12 D) 8 E) none of the above 94) Which of the following is a general trend for the electronegativity of elements in the periodic table? A) increases from left to right; increases from bottom to top B) decreases from left to right; increases from bottom to top C) increases from left to right; decreases from bottom to top D) decreases from left to right; decreases from bottom to top E) none of the above 94) ______ 95) According to the general trends in the periodic table, which of the f …
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