Grossmont College Name ______________________________Chemistry 141Vance Lab Day____________ Date ____________Chemistry 141: Final Exam Practice Question 1. When measuring a solid metal blockat constant temperature, whichmeasurement will change innumerical value depending on thelocation where it is taken?a) lengthb) massc) volumed) weighte) none of the above Question 2. Which of the following is the lowesttemperature?a) 37 °Cb) 54 °Fc) 313 Kd) all the temperatures are equal e) none of the aboveQuestion 3. Which of the following statementsdoes not describe a physicalproperty of chlorine?a) chlorine combines with sodiumto form table saltb) it is a green gasc) at STP its density is 3.17 g/Ld) freezing point is –101 °Ce) none of the above Question 4. A gold ingot weight 5.50 lbs. If thedensity of the gold is 19.31 g/cm3,and the length and width of the ingotare 12.0 cm and 3.00 cmrespectively, what is the height ofthe ingot?a) 6.50 x 10-3 cmb) 3.59 cmc) 10.2 cmd) 1.34 x 103 cm e) none of the aboveQuestion 5. The measured mass of a sample ofiron was 1.23 grams. Which digit inthe measurement has the leastcertainty?a) the first digit, 1b) the second digit, 2c) the third digit, 3d) all digits are certaine) none of the aboveQuestion 6. A sample of pure calcium fluoridewith a mass of 15.0 g contains 7.70g of calcium. How much calcium iscontained in a 45.0 g of calciumfluoride? a) 2.56 gb) 7.70 gc) 15.0 gd) 23.1 ge) none of the aboveQuestion 7. Which of the following statementsconcerning ionic compounds is true?a) Essentially all ionic compoundsare solids at room temperature.b) Ionic compounds do not containany covalent bonds.c) Ionic compounds contain thesame number of positive andnegative ions.d) The chemical formula for anionic compound must show anonzero net charge. e) all of the aboveQuestion 8. An element has two naturallyoccurring isotopes. One has anabundance of 37.4% and an isotopicmass of 184.953 amu, and the otherhas an abundance of 62.6% and amass of 186.956 amu. What is theatomic weight of the element? a) 185.702 amub) 185.954 amuc) 186.207 amu d) 186.956 amue) none of the aboveQuestion 9. The formula of dinitrogen trioxide isa) N(OH)3b) (NO3)2c) N2O2d) N3O2e) none of the aboveQuestion 10. By analogy with the oxoanions ofsulfur, H2TeO3 would be named a) hydrotellurous acidb) pertelluric acidc) telluric acidd) tellurous acide) none of the abovePage 1 of 8Grossmont College Final Exam ReviewChemistry 141 VanceQuestion 11. Record the following measurementto the correct number of significantfigures:a) 4.80 cmb) 5.13 cmc) 4.8 cmd) 4.00 cme) none of the aboveQuestion 12. How many protons, neutrons, andelectrons are in one atom ofmagnesium-23? a) 12, 12, 12b) 12, 11, 12c) 12, 23, 12d) 23, 23, 23e) none of the aboveQuestion 13. How many electrons are in thecarbonate ion?a) 16b) 28c) 30d) 32e) none of the above**Question 14. Which of the following statements istrue about ionic compounds?a) Essentially all ionic compoundsare solids at room temperature.b) Ionic compounds do not containany covalent bonds.c) Ionic compounds contain thesame number of positive ions asnegative ions.d) The chemical formula for anionic compound must show anegative charge.e) all of the aboveQuestion 15. If 5.98 g of sodium metal and waterreact to form 0.26 g of hydrogen gasand 10.40 g of sodium hydroxide,what mass of water was involved inthe reaction?a) 4.68 gb) 5.98 gc) 10.14 gd) 10.66 ge) none the aboveQuestion 16. Name the compound FeSO4:a) iron(II) sulfateb) iron sulfatec) ferrous sulfated) a and c onlye) all of the aboveQuestion 17. The chemical formula of potassiumperoxide is:a) KOb) KO2c) K2Od) K2O2e) none of the aboveQuestion 18. 8.0 g of iron is reacted with 8.0 g ofwater according to the chemicalequation shown below. Which oneof the following statements is false?3 Fe (s) + 4 H2O (l)  Fe3O4 (s) + 4 H2 (g)a) 11.1 g of Fe3O4 are producedb) 4.56 g of H2O are left overc) Mass is conserved in thisreaction.d) Iron is the limiting reactant.e) none of the above Question 19. What mass of sulfur hexafluoridehas the same number of fluorineatoms as 25.0 g of oxygendifluoride? a) 0.901 gb) 8.33 gc) 22.5 gd) 203 ge) none of the aboveQuestion 20. What is the concentration of nitrateions in a solution prepared bydissolving 30.0 g of calcium nitratein enough water to produce 300 mL?a) 0.305 Mb) 0.609 Mc) 0.806 Md) 1.22 Me) none of the aboveQuestion 21. What is the empirical formula of asubstance that contains 2.64 g C,0.444 g H and 7.04 g O?a) CH2O2b) C2H4O2c) C2H4O3d) C3H4O4e) none of the abovePage 2 of 8Grossmont College Final Exam ReviewChemistry 141 VanceQuestion 22. What is the atomic mass of 6Li, ifthe atomic mass of lithium is 6.941amu, and 7Li is 92.58% abundantand weighs 7.015 amu?a) 6.015 amub) 7.420 amuc) 0.074 amud) not enough informatione) none of the aboveQuestion 23. The mixing of which pair ofreactants will result in aprecipitation reaction?a) CsI (aq) + NaOH (aq)b) HCl (aq) + Ca(OH)2 (aq)c) K2SO4 (aq) + Ba(NO3)2 (aq)d) NaNO3 (aq) + NH4Cl (aq)e) all of the aboveQuestion 24. What is the oxidation half reactionin the chemical reaction:Zn (s) + 2 H+ (aq)  Zn2+ (aq) + H2 (g)a) Zn (s)  Zn2+ (aq) + 2 e-b) Zn2+ (aq) + 2 e-  Zn (s)c) 2 H+ (aq) + 2 e-  H2 (g)d) H2 (g)  2 H+ (aq) + 2 e-e) none of the aboveQuestion 25. Using the following portion of theactivity series for oxidation halfreactions, determine whichcombination of reactant will result ina reaction?Na (s)  Na+ (aq) + e- Cr (s)  Cr3+ (aq) + 3 e-a) Na (s) with Cr (s)b) Na (s) with Cr3+ (aq)c) Na+ (aq) with Cr3+ (aq)d) Na+ (aq) with Cr (s)e) none of the aboveQuestion 26. Based on the balanced chemicalequation shown below, determinethe mass percent of ferric ions in a0.6450 g sample of iron ore, if 22.40mL of a 0.1000 M stannous chloridesolution is required to completelyreact with the ferric ions present inthe ore sample. Given:2 Fe3+ (aq) + Sn2+ (aq)  2 Fe2+