Study Guide/Practice Exam for Chem 109 Exam 1
Study Guide/Practice Exam for Chem 109 Exam 1 CHEM 109
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This 12 page Study Guide was uploaded by Harley Hentges on Monday September 12, 2016. The Study Guide belongs to CHEM 109 at University of Nebraska Lincoln taught by Jason Kautz in Fall 2016. Since its upload, it has received 11 views. For similar materials see General Chemistry 1 in Chemistry at University of Nebraska Lincoln.
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Date Created: 09/12/16
CHEM 109 Fall 2016 Exam 1 Study Guide NAME THE FOLLOWING COMPOUNDS LiBr FeI3 Ni3PO4 MnO2 P5O10 (NH4)2CO3 Cu(CN)2 Sr(HSO3)2 PBr4 RbF NaNO3 NH4C2H3O2 NaHCO3 1 GIVE THE FORMULA FOR THE FOLLOWING COMPOUNDS sulfur dioxide calcium biphosphate hydrogen peroxide ammonium chloride chromium (III) carbonate nickel (I) acetate silicon tetrachloride cadmium (II) biphosphate cesium thiosulfate aluminum sulfide mercury (II) carbonate ammonium iodide copper (I) sulfate heptahydrate MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which of the following is a physical property? A) sulfur burns in oxygen to form sulfur trioxide B) ozone reacts with silver to give silver oxide C) the density of lead D) platinum metal does not react with hydrochloric acid 2 2) A chemical change always involves a change in: I) appearance II) state III) composition IV) temperature A) II and IV B) I and II C) I, II, IV D) III only E) all of the above 3) The term substance should be used for A) chemical elements, compounds, and mixtures B) any mixture. C) compounds D) chemical elements E) both chemical elements and compounds 4) Which one of the following would be classified as a heterogeneous mixture? A) salt water B) a sugar solution C) mix of table salt and black pepper D) copper nitrate solution E) brass 5) From ammonia gas, one can obtain two different gases, each of which is a pure substance. Using only this information, it can be said with certainty that: A) neither of the products can be an element B) gases do not produce solids C) both products are elements D) ammonia cannot be an element E) one of the products is an element 6) Which of the following is longest? A) 3.0 × 10^ ‒10 cm B) 3.0 nm C) 3.00 × 10^‒9 km D) 300 pm E) 3.0 × 10^‒4 m 3 7) Convert 82°F to the Kelvin scale. A) 245 K B) 301 K C) 452 K D) 373 K E) 195 K 8) If the density of aviation fuel is 1.77 lb/L, how many liters must be added to a tank to give 16,131 kg? (1 kg = 2.204 lbs) A) 2.01 x 104 L B) 1.30 x 104 L C) 1.30 x 103 L D) 1.61 x 104 L E) 9.11 x 103 L 9) An extensive property is A) difficult to measure B) independent of the quantity of matter observed C) is a unique value regardless of the measurement conditions D) dependent on the quantity of matter observed E) always strongly dependent on the external conditions 10) The following measurements were made by a group of students using the same balance and a 25.00 gram weight. Trial Mass (g) 1 23.96 2 24.01 3 23.98 4 23.97 The data would be considered: I) accurate and precise II) accurate but not precise III) precise but not accurate IV) neither precise nor accurate V) evidence of a systematic error VI) evidence of large random errors A) I only B) II and VI C) III and V D) IV and VI E) IV, V, VI 4 11) A 15.0 g sample of hydrated copper sulfate was heated to dryness and the new mass measured to be 9.59 g. Calculate the percentage of water in the hydrated crystal. Express your answer to the correct number of significant digits. A) 45% B) 63.3% C) 36% D) 63% E) 36.1% 12) A 25 g sample of sugar is found to contain 51.4% oxygen by mass. Another 250 g sample of the same sugar is also 51.4% oxygen by mass. This is consistent with the: A) law of constant composition B) law of conservation of mass C) law of multiple proportions D) second assumption of Dalton's theory E) first assumption of Dalton's atomic theory 13) When decomposed chemically, 73.0 grams of a sample of HCl produce 71.0 g of Cl2 and 2.0 g of H2, while 34.0 g of a sample of H2S produce 32.0 g of S and 2.0 g of H2. This is an example of the Law: A) of Definite Proportions B) of Simple Whole Numbers C) of Multiple Proportions D) of Conservation of Mass E) E = mc 2 5 14) Dalton's atomic theory is based on several assumptions, which are listed below. Which of these assumptions is strictly correct? I) All atoms of the same element are identical. II) Atoms are indivisible and unchangeable. III) Chemical changes are the result of the combination, separation, and rearrangement of atoms. A) I and II are correct. B) III is correct. C) I, II, and III are correct. D) II and III are correct. E) I and III are correct. 15) Which of the following statements is true concerning the masses of individual Cl atoms? A) All atoms have a mass of 35.45 u. B) All atoms have a mass of 17 u. C) None of the atoms have a mass of 35.45 u. D) Most of the atoms have a mass of 35.45 u. E) Some of the atoms have a mass of 35.45 u. 16) A hypothetical element, E, has two stable isotopes: E46 = 46.046 u 64.08% E51 = 50.826 u 35.92% What is the average atom weight of the element? A) 47.76 u B) 48.44 u C) 48.50 u D) 47.44 u E) 49.11 u 6 17) 57.7 g Ni contains how many atoms? A) 3.47 × 10^23 B) 5.92 × 10^23 C) 1.24 × 10^24 D) 0.983 E) 6.13 × 10^23 19) If the density of lead (Pb) is 11.34 g/cm^3 , how many atoms are in a piece of lead that is 2.00 cm wide, 1.00 m long, and 2.00 mm thick? A) 1.32 × 10^24 B) 6.60 × 10^23 C) 1.16 × 10^22 D) 1.16 × 10^23 E) 1.32 × 10^23 What is the mass of a Cl atom in atomic mass units? A) 35.00 u B) 35.45 u C) 34.97 u D) 36.36 u E) 13.95 u 20.) Aspartame, C14H18N2O5, a lowcalorie sweetener, is about 200 times sweeter than sugar. How many molecules of aspartame are there in a onegram packet of sweetener containing 36 mg aspartame? A) 7.2 × 10^25 molecules of aspartame B) 2.0 × 10^18 molecules of aspartame C) 7.4 × 10^19 molecules of aspartame D) 4.0 × 10^20 molecules of aspartame E) 1.4 × 10^22 molecules of aspartame 7 21) White phosphorus, P4, spontaneously bursts into flame in oxygen. If 6.500 g of white phosphorus reacts with oxygen to form 11.54 g of a phosphorus oxide, what is the empirical formula of this oxide? A) P4O6 B) P2O3 C) P2O6 D) PO3 22) When the equation Fe2(C2O4)3 → FeC2O4 + CO2 is balanced with the smallest integer coefficients, the coefficient of CO2 is: A) 1 B) 5 C) 4 D) 3 E) 2 23) How many grams of N2 are required to react with 2.30 moles of Mg in the following process? 3Mg + N2 → Mg3N2? (Mg = 24.3 g/mol, N = 14.0 g/mol) A) 0.767 g B) 193.2 g C) 21.5 g D) 0.027 g E) 64.4 g 24) In which of the following are the molecular and empirical formulas identical? A) NaCl B) CH4 C) C6H12O6 D) I2 E) both B and D are correct 8 25) 42.6 g Cu are combined with 84.0 g of HNO3 according to the reaction: 3Cu + 8HNO3 → 3Cu(NO3)2 + 2NO + 4H2O Which reagent is limiting and how many grams of Cu(NO3)2 are produced? A) HNO3, 93.8 g B) HNO3, 125.6 g C) Cu(NO3)2, 125.6 g D) Cu, 93.8 g E) Cu, 125.6 g 26) The Haber Process for the production of ammonia is represented by: 3H2(g) + N2(g) → 2 NH3(g) If a mixture of 30 g of hydrogen with 10 g of nitrogen produced 8.4 g of ammonia, what was the percent yield? A) 49% B) 20% C) 69% D) 28% E) 84% 27) Consider the gaseous reaction: N2H4(g) + 3O2(g) → 2NO2(g) + 2H2O(g) If the above reaction has a percent yield of 98.5%, what mass in grams of oxygen is needed to produce 49.0 g of NO2(g), assuming an excess of N2H4(g) ? A) 50.4 g B) 51.9 g C) 23.1 g D) 11.5 g E) 25.9 g 9 28) Which of the following is the correct formulation for the ammonium ion? A) NH4+ B) NO3– C) NO2– D) Am+ E) None of the above are correct 10 Answer Key: LiBr lithium bromide FeI3 iron (III) iodide Ni3PO4 nickel (I) phosphate MnO2 manganese (IV) oxide P5O10 p entaphosphorous decoxide (NH4)2CO3 a mmonium carbonate Cu(CN)2 copper (II) cyanide Sr(HSO3)2 s trontium bisulfite PBr4 phosphorous tetrabromide RbF rhubidium fluoride NaNO3 sodium nitrate NH4C2H3O2 ammonium acetate NaHCO3 sodium bicarbonate sulfur dioxide SO2 calcium biphosphate CaHPO4 hydrogen peroxide H 2O2 ammonium chloride NH4Cl chromium (III) carbonate Cr2(CO3)3 nickel (I) acetate NiC2H3O2 silicon tetrachloride SiCl4 cadmium (II) biphosphate CdHPO4 cesium thiosulfate Cs2S2O3 aluminum sulfide l2S3 mercury (II) carbonate HgCO3 ammonium iodide NH4I copper (I) sulfate heptahydrate Cu2SO4.7H2O 11 Answer Key: 1. C 2. D 3. E 4. C 5. D 6. E 7. B 8. A 9. D 10. C 11. C 12. A 13. D 14. B 15. E 16. A 17. B 18. A 19. B 20. A 21. B 22. B 23. B 24. E 25. C 26. C 27. B 28. A \ 12
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