MT1 practice 1 key

MT1 practice 1 key - All questions are worth 5 points...

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: All questions are worth 5 points 1. Which of the following measurements of length is shortest? a. 1.25 nm b. 12.5 µm c. 125 pm d. 12.5 Å e. 1.25x10–10 km 2. What is the temperature of liquid nitrogen in ˚F if its temperature is 77 K? a. –91 ˚F b. –247 ˚F c. –321 ˚F d. –411 ˚F e. 0 ˚F 3. Which mass measurement(s) must have exactly five significant figures? a. 1.0005 g b. 1.5000 g c. 15,000 g d. a and b e. a, b, and c 4. Which sum(s) of length measurements has exactly three significant figures? a. 1.25 m + 8.5 m b. 4.245 m + 8.5 m c. 5.55 m + 8.50 m d. b and c e. a, b, and c 5. What is the result of the calculation to the proper number of significant figures? 1005.34 m − 97.4 m = ? 125.68 s a. 7.2 b. 7.22 € c. 7.224 d. 7.2242 e. 7.22422 1 6. Convert the density of water of 1.00 g/mL to kg/m3 a. 0.1 kg/m3 b. 1.0 kg/m3 c. 1.00 x 102 kg/m3 d. 1.00 x 103 kg/m3 e. 1.00 x 106 kg/m3 7. Convert 1.25 nm to cm. a. 1.25 x 1011 cm b. 1.25 x 107 cm c. 1.25 x 10–7 cm d. 1.25 x 10–11 cm e. none of the above 8. Which of the following statements is true? a. The SI unit of length is the km b. The SI unit of mass is the gram c. The SI unit of energy is the calorie d. All of the above statements are true e. All of the above statements are false 9. What does the atomic number of an element specify? a. The number of neutrons in the nucleus b. The total number of neutrons and protons in a nucleus c. The number of protons in the nucleus d. The number of atoms in 1 gram of an element e. The number of different isotopes of an element 10. Which compound is formed between strontium ions and nitrogen ions? a. SrN b. Sr3N2 c. Sr2N3 d. SrN2 e. SrN3 2 11. What is the correct name of the compound with a formula of CaBr2? a. Bromine Calcide b. Calcium dibromide c. Calcium bromide d. Calcium bromine e. None of the above 12. What is the correct name of the binary compound with a formula of CBr4? a. Carbon tetrabromide b. Carbon tetrabromine c. Monocarbon tetrabromide d. Monocarbon tetrabromine e. Carbon (IV) bromide 13. What is the formula of the compound with a name of nitrous acid? a. HNO b. HNO2 c. HNO3 d. HNO4 e. HN2O 14. Which of the following is the formula of iron (III) oxide? a. Fe3O2 b. Fe2O3 c. FeO3 d. Fe3O e. Fe3O3 15. Which of the following ions has the same charge as the hydroxide ion? a. Ammonium b. Carbonate c. Nitrate d. Sulfate e. Phosphate 16. What is the % sodium in sodium carbonate? a. 21.7 % b. 27.7 % c. 36.1 % d. 43.4 % e. 55.4 % 3 17. Which of the following atoms have identical number of neutrons? a. 14C and 14N b. 12C and 13C c. 14C and 16O d. 16O and 18O2– e. None of the above 18. There are __________ electrons, __________ protons, and __________ neutrons in an atom of . a. 132, 132, 54 b. 54, 54, 132 c. 78, 78, 54 d. 54, 54, 78 e. 78, 78, 132 19. Rhenium (75Re) has two naturally ­occurring isotopes with atomic weights 184.9530 and 186.9560. What is the percent abundance of the lighter isotope? a. 62.60 b. 61.10 c. 39.90 d. 38.90 e. 37.40 20. The compound XF3, where the identity of X is unknown, was found to consist of 64.8% F by mass. What is the atomic weight of X? a. 14.0 amu b. 31.0 amu c. 35.5 amu d. 74.9 amu e. 79.9 amu 4 21. Aziridine contains only carbon, hydrogen and nitrogen. When a 0.4730 g sample is burned completely in oxygen, 0.9673 g of CO2 and 0.4916 g of H2O are formed. What is the empirical formula of aziridine? a. C2H5N b. C4H7N c. C3H7N2 d. C4H9N e. C5H7N 22. A compound composed only of carbon and hydrogen is 80.0 % C and 20.0 % H. The molecular weight of the compound is double the mass of the empirical formula. What is the empirical formula, molecular formula, and name of this compound, respectively? a. CH3, C2H6, ethane b. CH3, C2H6, ethanol c. C2H5, C4H10, butane d. C2H5, C4H10, butanol e. None of the above 23. What are the coefficients, respectively, when the following reaction is balanced? 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 24. The reaction in the preceding question (#23) is best classified as which type? a. Combination b. Oxidation ­Reduction c. Metathesis d. Acid ­Base e. Decomposition 5 25. Write the balanced chemical reaction for the reaction between solid magnesium and nitrogen gas to form magnesium nitride: " In a particular experiment, a 9.27 ­g sample of N2 (g) completely reacts. What is the mass of Mg (s) consumed during the reaction (in g)? a. 8.04 g ! b. 24.1 g c. 16.1 g d. 0.92 g e. 13.9 g 26. Sulfur and oxygen combine to produce sulfur trioxide: 2 S (s) + 3 O2 (g) " 2 SO3 (g) In a particular experiment, the reaction of 1.0 g S with 1.0 g O2 produced 0.80 g of SO3. What is the % yield in this experiment? (Hint: consider which reactant is the limiting reactant). ! a. 21 % b. 29 % c. 32 % d. 48 % e. 88 % 27. One mole of which substance contains the largest total number of atoms? a. S8 b. (NH4)3PO3 c. Al2(SO4)3 d. C10H8 e. One mole of all substances have the same number of atoms 28. What is the total concentration of ions in a 0.500 M Na2SO4 aqueous solution? a. 0.250 M b. 0.500 M c. 1.00 M d. 1.50 M e. ≥ 2.0 M 6 29. What are the spectator ions in the reaction of sodium chloride with lead nitrate? a. Na+ b. Na+ and Cl– c. Na+ and NO3– d. NO3– e. Cl– and NO3– 30. Which of the following reactions leads to the formation of a precipitate? a. Ca(OH)2 (aq) + CuCl2 (aq) b. Na2CO3 (aq) + Ca(NO3)2 (aq) c. CaI2 (aq) + FeSO4 d. a and b e. a, b, and c 31. How many of the following compounds are weak electrolytes in water? KOH Fe(OH)3 Ca(OH)2 RbOH Mg(OH)2 Al(OH)3 a. 0 b. 1 c. 2 d. 3 e. ≥4 32. A brick consisting of a pure metal measures to be 4.00 inches x 5.00 inches x 3.00 inches and weighs 7.020 kg. Using density, identify the metal in the brick. Metal Al Fe Ni Ti Zn Density (g/cm3) 2.70 7.86 8.91 4.50 7.14 a. b. c. d. e. Al Fe Ni Ti Zn 7 33. Which set(s) of values are NOT POSSIBLE for calcium, nickel, and lead? Set A B C a. b. c. d. e. Mass Number 40 58 82 Atomic Number 20 28 36 Number of Number of protons neutrons 20 20 28 30 36 46 Element Calcium Nickel Lead Set A Set B Set C All of the sets are correct All of the sets are incorrect 34. Which statement is true of all balanced chemical reactions? a. The mass of reactant(s) must equal mass of product(s) b. The moles of reactant(s) must equal moles of product(s) c. The concentration of reactant(s) must equal concentration of product(s) d. The molecules of reactant(s) must equal molecules of product(s) e. More than one of the above statements is true 36. Which of these metals is the least easily oxidized? a. sodium b. gold c. iron d. calcium e. silver 37. Which of the following statements is true for the combustion reaction of ethane. a. Carbon is oxidized and hydrogen is reduced b. Carbon is reduced and oxygen is oxidized c. Carbon is oxidized and oxygen is reduced d. Carbon is reduced and hydrogen is oxidized e. The reaction is not a redox reaction, so no atoms are oxidized or reduced 8 38. The molarity in mol/L could be calculated for a salt solution if which set of information was known? a. The mass of the salt added to the solution and the volume of water added to the solution. b. The mass of the salt added, the molar mass of the salt, and the total volume of the solution. c. The mass of the salt added to the solution and the total volume of the solution. d. The molar mass of the salt and the total volume of the solution. e. The mass of the salt added, the molar mass of the salt, the volume of the water added, and the total volume of the solution. 39. How many grams of phosphoric acid are there in 175 mL of a 3.5 M solution of phosphoric acid? a. 0.61 g b. 60 g c. 21 g d. 4.9 g e. 610 g 40. 0.400 L of an aqueous ethanol solution was diluted to a total volume of 4.00 L by adding water, giving a final concentration of 0.0400 M. What is the concentration of the original solution? a. 0.400 M b. 0.200 M c. 2.00 M d. 1.60 M e. 4.00 M 41. Consider the reaction: 2 MnO4– + 5 H2O2 +6 H+ → 2 Mn2+ + 8 H2O + 5 O2 What volume of 0.150 M KMnO4 solution is needed to completely react with 75.0 mL of 0.150 M H2O2? a. 15.0 mL b. 30.0 mL c. 45.0 mL d. 75.0 mL e. None of these 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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
View Full Document

Ask a homework question - tutors are online