Exam 4 Sample Problems
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Exam 4 Sample Problems

Course Number: CHEM 151, Spring 2008

College/University: Arizona

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10)The oxidation number for chromium in each of the following items respectively is: Cr2O7 A) +2, +2, +1 2- Cr2(SO4)3 C) +12,+3, +6 CrO3 D) +6,+3,+6 B) -2, 0, 0 16). (12 pts) Identify the type of each of the following chemical reactions using two terms for each: Use for set A Use for set B Single displacement Precipitation Double displacement Acid-base neutralization combustion Oxidation-reduction...

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oxidation 10)The number for chromium in each of the following items respectively is: Cr2O7 A) +2, +2, +1 2- Cr2(SO4)3 C) +12,+3, +6 CrO3 D) +6,+3,+6 B) -2, 0, 0 16). (12 pts) Identify the type of each of the following chemical reactions using two terms for each: Use for set A Use for set B Single displacement Precipitation Double displacement Acid-base neutralization combustion Oxidation-reduction decomposition Gas forming combination Complete but do NOT balance the equations then use TWO terms to name each reaction Set A Set B a. ZnCO3 ______+ _______ _____________ ______________ _______________ _______________ ______________ b. Ca + O2 ____ c. CH3 COOH + KOH ______+ _______ _____________ Complete the following table AND put an X in the box so show if the compound is soluble or insoluble name formula soluble insoluble copper (II) chloride Lithium carbonate Copper(II)sulfate X(free ) pentahydrate General group name:( RCOOH low molar mass ) HBrO3 (NH4)3PO4 ------------------------------------------------------------------------------------------------------------------------------- 3) Balance the following equation. ____Mg3N2 + ____H2SO4 ____MgSO4 + ____(NH4)2SO4 The SUM of all the coefficients (both reactants and products) is: a) 4 b) 6 c) 12 d) 9 e) 18 4) In the reaction Na + H2O NaOH + H2 The oxidizing agent is: A) Na B) H2O C) NaOH D) H 2 E) not a REDOX 5) Compounds A and B both contain Carbon, Hydrogen and Oxygen. They were tested using a light bulb conductivity apparatus and the results are recorded. Solution: Light Bulb Observation: Pure liquid A Does not light up Pure Liquid B Does not light up Liquid A dissolved in water Does not light up Liquid B disso in water Dim Which describes the compounds? A) A is ionic; B is a strong acid is a weak acid C) A is weak acid ; B is strong acid B) A is a soluble non-electrolyte: B D) A is covalent ; B is an alcohol 10) In the reaction A 2B You calculate that to reach a theoretical yield of 20 moles of B you need 10 moles of A . If the reaction has only a 75% yield how many moles of A must you react initially to achieve your original theoretical yield of 20 moles of B. A) 10 moles E) need more data. B) 7.5 mole C) 13.3 moles D) 15 moles 13) Write out the NET IONIC EQUATION for the reaction in water: 2 HNO3 + K2CO3 2KNO3 + H2CO3 (hint write out the entire reaction with ions) _______+_______+_______+______==> _______ + ________+_______+______(no graded points) The SPECTATOR IONS are: A) K1+, NO31B) CO32-, H1+ spectators C) H1+, OH 1- D) There are no 17) (15pts) Identify the type of each of the following chemical reactions using two terms for each: Use for set A Use for set B Single displacement Precipitation Double displacement Acid-base neutralization combustion Oxidation-reduction decomposition Gas forming combination No reaction (NR) No reaction (NR) Complete but do NOT balance the equations then use TWO terms to name each reaction NR No Reaction is always a possibility. 15 points one for each blank. Set A A) ZnCO3 + HNO3 _________+ _______+_______ _______________ B) Mg + S8 ____ ______________ _____________ Set B _______________ C) _________ + 2_______ Na2SO4+ H2O _____________ _______________ D) He 18) (13pts) + Ne __________ ______________ ________________ Given the following balanced reaction 2Al+ Fe2O3 2Fe + Al2O3 H = -850 kJ You mix 127g Al (MM= 26.98g/mol) with 265 g of Fe2O3 (MM= 159.7g/mol). What is the maximum yield of iron you can expect in grams? (show work for credit) MM Fe = 55.85 g/mol 5pts Yield= g Which reactant is the limiting reagent? Limiting reagent 3pts Complete the following table AND circle the information about the compound name formula ionic covalent P O Lithium perchlorate Calcium sulfate dihydrate General group name:( ) If C2O4 then 24 10 RCOOH low molar mass soluble free soluble Strong acid soluble insoluble X(free) insoluble Weak acid insoluble is the oxalate ion Oxalic acid = (NH4)3PO4 Grade _____/100 1)(10 points) From OWL Nitrogen monoxide (NO) is produced by combustion in an automobile engine. For the following reaction, 0.235 moles of nitrogen monoxide are mixed with 0.313 moles of oxygen gas. nitrogen monoxide (NO) (g) + oxygen (O2) (g) Write the Balanced equation: (2pts) + ===> nitrogen dioxide (NO2)(g) What is the FORMULA for the limiting reagent? What is the maximum amount of NO2 that can be formed? 4pts moles 4pts 2) 6 points following:. SF6 Compute the oxidation number for S only in each of the H2SO4 S ox # = _____ 2pt S8 S ox # = ___________2pt S ox # = _____ 2pt _______________________________________________________________________ 3)( 6 points) From OWL Pb2+ + H2S Pb + S + 2 H+ In the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent. name of the element oxidized: name of the element reduced: formula of the oxidizing agent: formula of the reducing agent: 2 pts 2 pts 1 pts 1pts 4) 4pts Balance the reaction : Put in 1 if it is a coefficient ______S8 + _____ CO ==> SO2 _______ + _______ C 5) (8 pts) Complete and BALANCE the following reactions NO REACTION (NR) is always possible Mg (OH)2 + HBrO4 ===> ____________ + ______________ MgCO3 ===> ____________ + ______________ NiCl2 + Na2S Na2CO3 + HBr ===> ____________ + ______________ ===> ____________ +_____________+__________ 6)( 4 pts) MATCH the TYPE of the following reactions (use the following names ONLY ONCE : precipitation, neutralization (acid/base), REDOX, thermal decomposition, gas forming - ) NO REACTION (NR) is always possible He + Ne ===> ? reaction type ___________________ 1111NO3 + ClO3 NO2 + ClO4 reaction type ____________________ HBr(aq) + NaOH(aq) ==> NaBr(aq) + H2O reaction type ____________________ 2AgNO3 + Na2S ===> Ag2S (s) + 2 NaNO3 reaction type ____________________ ________________________________________________________________________ ___ 7)(10pts) In the laboratory you dissolve 17.7 g of cobalt(II) fluoride CoF2 (MW = 97) in a volumetric flask and add water to a total volume of 250 mL. What is the molarity of the solution ? M. 5pts M. 3pt M. 2pts What is the concentration of the cobalt(II) cation ? What is the concentration of the fluoride anion ? 8)(3 pts) Which picture illustrates the behavior of the CaCl2 in a water solution? Circle 9) (10 pts) Substance HNO3 HNO2 Put an X in the correct column (pick only one per substance) Strong electrolyte Weak electrolyte Non-electrolyte or insoluble CH3CH2CH2OH NaC9H16O11 AgCl Classify the following substances: place a number from the right in a box on the left 1) strong acid HCl 2) weak acid NaCl 3) strong base Cr2(CO3)3 4) weak base 5) salt: soluble KOH 6) salt: not soluble HCOOH 10) (6 pts) Write out the NET IONIC EQUATION for the reaction: Ni(NO3)2 + Na2S NiS (s) + 2NaNO3 answer _______+_______==> _______________ 1. Balance the following equations with the lowest possible whole number coefficients: a. ___C5H10O2(l) + ___O2(g) ___CO2(g) + ___H2O(l) b. ___Al(OH)3(s) + ___H2SO4(aq) ___Al2(SO4)3(aq) + ___H2O(l) 2. Automotive airbags inflate when sodium azide rapidly decomposes to its component elements: 2NaN3(s) Na(s) + 3N2(g) How many grams of NaN3 are required to form 5.00 g of nitrogen gas? NaN3 = 65.00999 amu, N2 = 28.01348 amu 1. How many grams of carbon dioxide can form when a mixture of 4.95 g ethylene (C2H4) and 3.25 g of oxygen gas is ignited according to the following equation? C2H4(g) + 3O2(g) 2CO2(g) + 2H2O(g) What is the limiting reactant? How many grams of the excess reactant remain? C2H4 = 28.0532 amu, O2 = 31.9988 amu, CO2 = 44.0095 amu Limiting reactant: _____________ _________________ Mass of CO2 formed: Mass of excess reactant left:_________________ 3. What is the oxidation number of each element in: a. Ca(OCl)2 Ca = _____ b. HPO42O = _____ Cl = _____ H = _____ P = _____ O = _____ 4. Identify the type of reaction: precipitation, acid-base, redox, combination, single replacement, double replacement, decomposition, and/or combustion. (A reaction can be more than one type give all possibilities.) a. When solid sodium reacts with oxygen gas, solid sodium oxide is formed. b. When solutions of sodium chloride and silver nitrate are mixed, a cloudy precipitate of silver chloride forms, along with aqueous sodium nitrate. c. C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(g) d. HBrO2(aq) + NaOH(aq) H2O(l) + NaBrO2(aq) 5. Balance the following equations with the lowest possible whole number coefficients: a. ___C5H6O(l) + ___O2(g) ___CO2(g) + ___H2O(l) b. ___Cr(OH)3(s) + ___HClO4(aq) ___Cr(ClO4)3(aq) + ___H2O(l) 6. Hydrofluoric acid, HF(aq), cannot be stored in glass bottles because compounds called silicates in the glass are broken down by the HF. One example: Na2SiO3(s) + 8HF(aq) H2SiF6(aq) + 2NaF(aq) + 3H2O(l) How many grams of NaF form when 3.50 g of HF react in this way? HF = 20.00634 amu, NaF = 41.988173 amu 1. How many grams of carbon dioxide can form when a mixture of 2.99 g propylene (C3H6) and 4.50 g of oxygen gas is ignited according to the following equation? 2C3H6(g) + 9O2(g) 6CO2(g) + 6H2O(g) What is the limiting reactant? How many grams of the excess reactant remain? C3H6 = 42.0797 amu, O2 = 31.9988 amu, CO2 = 44.0095 amu Limiting reactant: _____________ Mass of CO2 formed: _________________ Mass of excess reactant left:_________________ 1. Write balanced molecular equations and net ionic equations for the following reactions in aqueous solution. If no reaction occurs, write NR. (Don't forget phase labels) a. NaNO3(aq) + Pb(C2H3O2)2(aq) b. HBr(aq) + Al(OH)3(s) c. AgNO3(aq) + KI(aq) d. A solution of hydrochloric acid is mixed with a solution of rubidium sulfite 7. What is the oxidation number of each element in: a. Cr(OH)4 Cr = _____ b. Ca(NO3)2 Ca = _____ N = _____ O = _____ O = _____ H = _____ 7. Barium sulfate is made by the following reaction Ba(NO3)2(aq) + Na2SO4(aq) BaSO4(s) + 2NaNO3(aq) An experiment was begun with 75.00 g of Ba(NO3)2 and an excess of Na2SO4. After collecting and drying the product, 63.45 g of BaSO4 was obtained. Calculate the percent yield of the reaction.

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