MT1 practice 2

MT1 practice 2 - Practice MT1, AU10. Section I....

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Unformatted text preview: Practice MT1, AU10. Section I. Sig. figs., dimensional analysis, units: Each question is worth 3.5 points 1. How many significant figures are in the value 0.01005020 seconds? a. 9 b. 8 c. 7 d. 6 e. 3 2. Complete the following math operation. Report answer with proper sig figs. 9.35 m + 3.4 m = a. 12.75 m b. 12.8 m c. 13 m d. 1.3 x 101 m e. none of the above 3. How many significant figures are in the result of the calculation: (9.75 m+1.25 m)/2.1255 sec = a. 1 b. 2 c. 3 d. 4 e. 5 4. Convert 0.825 pounds to grams. a. 0.374 g b. 1.82 g c. 374 g d. 1.82 x 103 g e. 4.72 x 104 g 1 5. Convert 525 ps to seconds. a. 5.25 x 10–12 s b. 5.25 x 10–10 s c. 5.25 x 10–7 s d. 5.25 x 1012 s e. 5.25 x 1014 s 6. Convert 5.25 x 104 cm2 to m2. a. 5.25 m2 b. 525 m2 c. 5.25 x 104 m2 d. 5.25 x 106 m2 e. 5.25 x 108 m2 7. Convert 0.0105 g/cm3 to g/L. a. 100.5 g/L b. 10.5 g/L c. 1.05 g/L d. 0.0105 g/L e. 1.05 x 10–5 g/L 8. Which of the following is the SI unit of mass? a. Joule b. Pound c. Milligram d. Gram e. Kilogram 2 Section II. Naming compounds: Each question is worth 3 points 9. What is the name of PO33–? a. Phosphite b. Phosphate c. Perphosphate d. Phosphide e. Phosphorus trioxide (III) 10. What which of the following is cerium(II) cyanide? a. Ce2CN b. Ce(CN)2 c. CeCN2 d. Ce2(CN)2 e. Ce2CN2 11. What is the name of NH4BrO3? a. Ammonia bromate b. Ammonium bromate c. Ammonia bromite d. Ammonium bromite e. None of the above 12. Which of the following is chromium(VI) nitrite? a. Cr(NO3)6 b. Cr6NO3 c. Cr6NO4 d. Cr6NO2 e. Cr(NO2)6 3 13. Which of the following compounds is a binary compound? a. HClO2 b. C2H5OH c. P4O10 d. N2 e. Both c and d 14. Which of the following is hydrosulfuric acid? a. HS b. H2S c. H2SO3 d. H2SO4 e. none of the above 15. What is the molecular formula of magnesium dihydrogen phosphate? a. Mg2HPO4 b. MgHPO4 c. Mg(H2PO4)2 d. Mg2(H2PO4)3 e. Mg3(H2PO4)2 16. Which of the following formula and name pairs are INCORRECT? I. HCl, chloric acid II. HClO, hypochlorous acid III. HBrO4, hypobromous acid IV. HNO2, nitrous acid V. H3PO3, phosphoric acid a. I, III b. III, V c. I, II, IV d. I, III, V e. II, IV 4 Section III. General questions: Each question is worth 6.15 points 17. What is the mass of one molecule of CO2 in grams? a. 4.40 x 10–22 g b. 44.0 g c. 7.31 x 10–23 g d. 1.66 x 10–22 g e. 5.12 x 10–21 g 18. Which experiment determined the mass and charge of an electron? a. Thompson’s Cathode ray tube experiment b. Rutherford’s gold ­foil experiment c. Dalton’s atomic theory d. Millikan’s oil ­drop experiment e. Currie’s experiment on radioactivity 19. How many neutrons does a cesium ­133 atom contain? a. 133 b. 78 c. 55 d. 42 e. Not enough information is provided 20. What is the chemical symbol of an atom with 20 neutrons, 20 protons, and 18 electrons? a. 20Ca2+ b. 40Ca2+ c. 20Zr2+ d. 40Zr2+ e. 40Ar2– 5 21. Consider the reaction between N2 represented by the black spheres and O2 represented by the grey spheres to produce NO2. N2 (g) + 2 O2 (g) " 2 NO2 (g) ! If the reaction proceeds to 100% yield, what molecules would be present in the box? a. 8 NO2 molecules b. 6 NO2 molecules c. 8 NO2 molecules + 1 O2 molecule d. 6 NO2 molecules + 1 N2 molecule e. None of the above 22. Determine the coefficients required to properly balance the following reaction. What are the coefficients of the balanced reaction from left to right, respectively. ___ Al(NO3)3 + ___ Na2S " ___ Al2S3 + ___ NaNO3 a. 2, 1, 1, 2 b. 2, 3, 2, 3 c. 1, 3, 1, 3 d. 2, 3, 1, 6 ! e. 4, 6, 2, 12 23. What is the empirical formula of a substance that is 53.3 % S, 40.0 % C, and 6.7 % H by mass? a. C2H4S b. C4H8S2 c. CH2S d. C6HS8 e. None of the above 6 24. A 1.084 g of a substance containing C, H, and N is combusted and yields 2.507 g CO2 and 1.287 g H2O. What is the percent nitrogen by mass of the substance? a. 23.6 % N b. 30.2 % N c. 33.3 % N d. 56.2 % N e. 88.9 % N 25. Which statement below is true when 3.75 g magnesium nitride and 3.2 g of water are reacted according to: Mg3N2 + 3 H2O " 2 NH3 + 3 MgO a. Magnesium nitride is the limiting reactant and water is the excess reactant. b. Water is the limiting reactant and magnesium nitride is the excess reactant. c. Water and magnesium nitride are both limiting reactants. d. Water and magnesium nitride are both excess reactants. ! e. The yield of MgO is limited by the amount of excess reactant present. 26. Which of the following compounds are strong electrolytes in water? FeCO3 KOH ZnCl2 Ag2S Pb(NO3)2 Hg2I2 Rb2S a. All compounds are soluble in water b. KOH, ZnCl2 c. ZnCl2, Rb2S d. KOH, ZnCl2, Pb(NO3)2, Rb2S e. KOH, ZnCl2, Pb(NO3)2, Hg2I2, Rb2S 7 27. Which of the following is the NET ­IONIC EQUATION for the metathesis reaction between Na3PO4 and Fe(NO3)2 in water? a. 3 Fe (s) + 2 PO43–(aq) " Fe3(PO4)2 (s) b. 3 Fe (aq) + 2 PO43–(aq) " Fe3(PO4)2 (s) c. 3 Fe2+ (aq) + 2 PO43–(aq) " Fe3(PO4)2 (s) d. 3 Fe2+ (aq) 6 NO3– (aq) + 6 Na+ (aq) + 2 PO43–(aq) " ! Fe3(PO4)2 (s) + 6 Na+ (aq) + 6 NO3– (aq) ! e. 3 Fe(NO3)2 (aq) + 2 Na3PO4 (aq) " Fe3(PO4)2 (s) + 6 NaNO3 (aq) ! 28. In each of the following instances two aqueous solutions are mixed. Which ! reaction will lead to the formation of a precipitate? a. sodium chloride solution + calcium hydroxide solution ! b. hydrochloric acid solution + sodium hydroxide solution c. aluminum nitrate solution + sodium chloride solution d. ammonium sulfide solution + zinc sulfate solution e. None of the above reactions will lead to formation of a precipitate 29. The metathesis reaction of aqueous solutions of BaI2 and CuSO4 yields a precipitate of BaSO4. Which ion(s) is/are spectator ions in the reaction? a. Ba2+ only b. Cu2+ only c. Ba2+ and SO42 ­ d. Cu2+ and I ­ e. I ­ only 30. Which solution has the greatest concentration of ions? a. 0.5 M NaCl in water b. 0.5 M FeCl3 in water c. 0.5 M K3PO4 in water d. 0.5 M Fe2(SO4)3 in water e. All solutions a ­d have the same concentration of ions. 31. Which of the following substances is NEITHER a strong acid nor a strong base? KOH HNO2 Al(OH)3 H2SO4 HClO NH3 HCl a. Al(OH)3 b. HNO2, Al(OH)3, HClO c. HNO2, Al(OH)3, NH3 d. HNO2, Al(OH)3, HClO, NH3 e. KOH, HNO2, Al(OH)3, HClO, NH3 8 32. What is the oxidation number of phosphorus in K3PO4? a. 2 b. 3 c. 4 d. 5 e. 6 33. Zinc metal can be _____________ to Zn2+ by the substance ______________ in water? a. Oxidized, Ca(CH3COO)2 b. Reduced, Ca(CH3COO)2 c. Oxidized, AgNO3 d. Reduced, AgNO3 e. Both b and c 34. How much water (in mL) must be added to 5.54 mL of 12.0 M HCl in water to yield a 1.00 M HCl solution? a. 66.5 mL b. 60.9 mL c. 45.4 mL d. 40.0 mL e. 21.6 mL 35. If 258 mL of a 0.500 M AgNO3 solution is mixed with 500 mL of a 0.312 M NaCl solution, what is the identity and mass of the precipitate that is formed? a. b. c. d. e. Precipitate = AgCl, mass = 18.5 g Precipitate = NaNO3, mass = 11.0 g Precipitate = AgCl, mass = 26.5 g Precipitate = AgCl, mass = 53.0 g Precipitate = NaNO3, mass = 13.3 g 36. The concentration of sulfuric acid in an automobile battery can be determined by titration. If a 25.00 mL sample of sulfuric acid solution of battery acid requires 87.42 mL of 1.95 M NaOH to reach the end ­point, what is the concentration of the battery acid (in M)? a. 1.70 M b. 3.41 M c. 4.22 M d. 5.42 M e. 6.82 M 9 Useful Information 1 gallon = 3.7854 L, 1 kg = 2.2046 lb., 1 inch = 2.54 cm, 1 mL = 1 cm3, 1 Å = 1x10–10 m NA = 6.022 x 1023, 1 amu = 1.66054 x 10–24 g, 1 g = 6.02214 x 1023 amu Solubility Tables Water soluble compounds contain: Exceptions: Acetate None Nitrate None Iodide, Bromide, and Chloride Compounds of Ag+, Hg22+, and Pb2+ Sulfate Compounds of Sr2+, Ba2+,Hg22+, and Pb2+ Water insoluble compounds contain: Exceptions: Sulfide, Hydroxide Compounds of the alkali metal cations, Ca2+, Sr2+, Ba2+, and NH4+ Carbonate, Phosphate Compounds of the alkali metal cations, and NH4+ 10 !"#$%&$'()*+,"(%-(./"(0,"1"2.3 611HIJJG6,.201789K3)419G). $%&!&'()**'+,-.,/012/, "3)41'56,.20178 =" <" >" > ? : 6 7 8 !" ! 4 !9&&:;< %" = < 5$ 6" ?9;<! ;9&!%!#% !&9#!! !%9&!&: !! !% != !< 8* ;< =, %%9;#;:?; %<9=&>& =@ <@ >@ ?@ :@ !@ %@ !; %& %! %% %= %< %> %? %: %# %; =& ? 7* >' )$ @ 7# ;2 :" 7% 8$ 7A =;9&;#= <&9&:# <<9;>>;!% <:9#?: >&9;<!> >!9;;?! ><9;=#&<> >>9#<> >#9;==!;> >#9?;=< =: =# =; <& <! <% <= << <> <? 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This note was uploaded on 11/28/2011 for the course CHEM 121 taught by Professor Wyzlouzil during the Spring '07 term at Ohio State.

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