Honors Chemistry Final Exam Study Guide 21-22 PDF

HONORS CHEMISTRY FINAL EXAM STUDY GUIDE 21-22 • • • • • TIPS FOR THE FINAL Review past chapter tests from 2nd semester. Do practice problems! Your packets have plenty of extra review problems, and you can check your answers with me anytime before the final. Study with a buddy! Quiz each other on de...

HONORS CHEMISTRY FINAL EXAM STUDY GUIDE 21-22 • • • • • TIPS FOR THE FINAL Review past chapter tests from 2nd semester. Do practice problems! Your packets have plenty of extra review problems, and you can check your answers with me anytime before the final. Study with a buddy! Quiz each other on definitions, concepts, laws, etc. Although this final covers material learned during the 2nd semester, it is expected that you know and can use concepts learned during the 1st semester such as ionic and covalent formulas, polarity, predicting products and balancing equations, etc. Start studying NOW! (THIS FINAL IS 10% OF YOUR SEMESTER 2 GRADE) DISCLAIMER: This study sheet is meant to be an indication of what is most likely to appear on the final exam. It does not in any way exempt other material, not listed here, to appear on the exam. However, the majority of concepts encountered on the exam are likely to be found here. • • • • • Reactions Identifying Types of Reactions and Predicting Products Balancing Equations Reaction diagrams Calorimetry Predicting shifts in equilibrium due to stresses applied (Le Chatelier’s Principle) • • • • • • • • • The Mole Atomic mass Mole Avogadro’s number Molar mass Empirical formula Molecular formula Percent composition Conversions among: grams, moles, particles Determining empirical formula and molecular formula • • • • • • • Interpreting balanced chemical equations Coefficients = number of moles and are used as mole ratio Mole to mole problems, Mass to mole problems, Mass to mass problems Limiting reactant Theoretical yield Percent yield – know formula Combustion analysis • • • • • • • Kinetic molecular theory 4 variables: amount of gas, volume, temperature, and pressure Gas pressure - define and unit conversions Atmospheric pressure STP is 1 atm and 273 K Gas laws: Avogadro, Boyle, Charles, Dalton, Ideal gas law Gases and stoichiometry Stoichiometry Gases Liquids and Solids • 3 types of intermolecular forces • • • • • • • • physical properties of solids, liquids, gases intramolecular vs. intermolecular unique characteristics of water viscosity and surface tension names of changes of state boiling vs evaporation heating curve phase diagram • • • • • • • • • • • • • What is a solution? Parts of a solution- solute and solvent Definitions What is an aqueous solution? Solubility graphs: both reading and manipulating data Molarity: formula and solving problems Saturated, unsaturated, and supersaturated solutions How a solution forms: solvation, dissociation, energy Like dissolves like Solubility of solids/gases Rate of dissolution Solutions and stoichiometry Total Ionic and Net ionic equations Solutions Acids and Bases • • • • • • • • • Nomenclature Arrhenius Bronsted-Lowry definitions Conjugate acid/base pairs Indicator Characteristics of acids and bases Buffers pH scale and calculations strong acid and bases titrations HONORS CHEMISTRY FINAL REVIEW 21-22 You will be given a periodic table, a gas laws formula sheet, solubility curve Unit 6: Chemical Reactions 1. Identify reactants and products and well as the state in the chemical equation below. AgBr(aq) + NaCl(aq) → AgCl(s) + NaBr(aq) reactants dissolved products intro 2. s solid precipitate aqin aqueous What do the coefficients mean a chemical equation? thatreactto maintainthelaw atomsormolecules formulaunits of conservation Coefficients matter Indicates ofmolesofea reactantproduct of 3. Balance and identify the ofreaction type of the following equations. a. ___Ag + ___N2 6 → ___Ag 3N 2 Type: ____________ S b. ___Na + ___F2 2 → Type: ____________ S c. ___Li 2 2O 2 + ___H ___NaF 2 → ___LiOH + ___H2 2 Type: ____________ d. ___C 2 4H10 + ___O2 → 8___CO Type: ____________ 13 2 + 10 ___H2O e. ___KOH + ___CuSO4 2 f. ___H 2 2 O2 g. ___Mg + ___Cl2 → ___MgCl2 h. ___Na 2 2 2 2O + ___Cl → ___O2 + ___NaCl → SR ___Cu(OH)2 + ___K2SO4 DR Type: ____________ D ___H 2 2O + ___O2 → C Type: ____________ Type: ____________ S SR 4 Type: ____________ 4. What type of reaction only has one product? Synthesis 5. What type of reaction has two compounds for reactants and two compounds as products? Doublereplacement 6. What number associated with compounds can you NEVER change? Why? Subscript Youwouldchangethe ofthe compound formula 7. Consider the following equilibrium: CH4(g) + H2O(g) + heat ⇄ CO(g) + 3 H2(g) Name and explain all possible stresses that shift the equilibrium to the right (adding or removing substances, heating or cooling, changing pressure, etc). AddcityorH2O dpressure 8. Consider the reaction: Zn + 2 HCl → ZnCl2 + H2 ΔH= -80.7 kJ/molrxn a. Is this reaction endothermic or exothermic? Explain. b. Sketch a reaction diagram for this reaction, labeling the activation energy, activation energy of reverse reaction, ΔH, products, reactants, and axes labels. j peo Ea TH sa ran progress c. If 10.0 grams of zinc was reacted with excess HCl, how much heat would be released? lo.ogznxjagxgzfx.gg 12.3kt 12.3ktwouldbereleased d. Assume all of the heat in part c was absorbed by 250.0 g of water. How much did the temperature change? The specific heat of water is 4.18 J/g℃. 12.34555 50 14.1852 At DE ii soc 9. Predict the products of the following reactions and balance: a. ____Na 2 + ____Cl2 → NaCl 2 b. ____NaOH + ____H2SO4 → 2 c. ____Li 2 + ____H 2 2O → 2Li ont d. ____Mg + ____HCl → 2 e. ____MgCO3 → 504 2H2o Naz Hz MgdatHz MgO t CO2 f. ____C4H10 + ____O 13 2 → 8Coat 10420 The Mole and Stoichiometry 1. What is a mole? 6021023items 2. Calculate the molar mass of a. C3H8O 3 12.014840111 1661,3 60igad b. Mg(OH)2 I 24.311,7 21161 211.011 58.33g 3. Perform the following calculations a. 5.5 mole of Pb has what mass? How many atoms? 5 5mdPbx 2 Pb 1100g 5.5ns 69 10atons 3.3 1024atoms b. 2.5 x 1013 formula units of NaHCO3 has what mass? c. What is the mass of 3.20 moles of Zn(NO3)2? b 2.5 10 fnNaHcO3xÉtgx 1 tl c 3romoltnlnoslzx 9 3.5 10 Znnos 606g 4a. Calculate the number of moles in 19.0 grams of MgO. 19OgMgOx 5g 471 melMgO b. Calculate the number of moles in 5.46 x 1022 molecules of C6H5Cl. molesColts Ctx 5 461022 me melCattell 0907 5. What is the % composition of each element in C3H6O3? %C 39.99 2 81 100 %H 64 44 %O 3 5 100 6.73 1 100 53 28 6. What is the molecular formula of a compound that has a molecular mass of 60.06 g/mol and is 40.0%C, 6.7%H, and 53.3%O. Fg Cx 40.0g 69 5330 4 3.33 mil 3zz g6mg EMP CHLO MMen530.03g if Mt 3.334 City 2 C4207 7. Consider the reaction: 4 P + 5 O2 → 2 P 2 O 5 If 25 g of phosphorus is reacted with excess oxygen, how many grams of P2O5 are formed? 25gPx It 205x 57g1205 thatgetsusedup in 8. Define limiting reagent. Thereactant theTY a reaction It alsodetermines 9. What is Avogadro’s number? How is it used in conversions?6.021023tv 6o2x103particles 10. A compound was analyzed and found to contain 13.5 g Ca, 10.8 g O, and 0.675 g H. What is the empirical formula for the compound? lmo 13.5gcaxHog 337mg 10.8g 675 1 337 675g 668m11 337 Ogl caLOH 2 I 2 2 g 11. Use the equation to answer the following questions: N2 H4 + 2 H2 O2 → N2 + 4 H2 O a. How many moles of N2H4 are represented by the equation? I b. How many moles of H2O2 are represented by the equation? 2 c. How many moles of H2O are represented by the equation? 4 d. What are the numbers in front of elements or compounds in a chemical equation called?coefficients e. How many moles of N2 are formed when 2.3 moles of H2O2 are reacted? 2 3mAH2O2x É 1.15mA N2 13. Determine the mass of sodium hydroxide (NaOH) produced when 0.25 g of sodium reacts with water according to the following equation: (Don’t forget to balance the equation) ____Na + ____H2O → ____NaOH + ____H2 2 22.5g o ga 28Naxgggxgreatx4g 14. Define theoretical yield. conditions 439 Themaximumamountofproduct thatcanbeformedunder It is determinedbythelimitingreactant pe fect 15. What is percent yield and how is it determined? ATIF t amount productformedw respectto the maximum of x 100 dyield thatcouldbeformed 16. In a reaction of 15.3 g of NaCl with 60.8 g Pb(NO3)2 a. Write a balanced chemical equation. 2NaCl Pb00312 Pbda t 2Nang b. How many grams of PbCl2 will be produced? Iggy Iggy 1 1513gNaClx x x 9 364gPbdz 60.8gPbN332x kgxyyjgf.gg 2g c. What is the limiting reagent? x 51.0g Pbda NaCl 364g d. What is the theoretical yield? e. How much excess reagent is left over? NO3 2 X Iggy jyffb 1513gNaclx x 60.8g 43.49 33 17.4gXSPbNO 43.4gused f. What is the percent yield if 32.3 g of lead (II) chloride is produced in the reaction? 3314 100 88.79yield 17. The combustion of 1.38 grams of a compound which contains C, H, O and N yields 1.72 grams of CO2 and 1.18 grams of H2O. Another sample of the compound with a mass of 22.34 grams is found to contain 6.75 grams of O. What is the empirical formula of the compound? CxHyOzN 138g CO2 H2O 02 1.72gcoaxtgxtco 118GHzOxFoggx 1.18g 1.72g II 431 469C htt I I 13294 100 34.0 0 91334 0 N 100 34.0 C 2.83 34.0gCx of 41534 100 30.21 0 30.27 2629N 1.5 2 3 H 959gHxf 9.50mg 5 0 30.21g Oy 1.89 N 26.29Nx tg 9.59 100 9.59 4 87 1.87mg 2 1 2 10 2 1 2 2 1341002Mt Gases 1. What causes pressure? Explain using KMT. If the temperature increases, what happens to the pressure of a gas, assuming all other variables are held constant? Pcaused collisions molee the container w g as of collisions w the speed molec I sothere are more If TTby of container causingT P 2. Describe the relationship in the following laws, state the mathematical equation, and state which variables must be held constant. a. Boyle’s Law b. Charles’s Law c. Avogadro’s Law d. Gay-Lussac’s Law constant PV PV2 n t YE p n P T E V Ez n 3. The unit of temperature for any of the gas laws is _____________!!!!!!!!!!!!!! KELVIN 4. The unit of pressure for the ideal gas law is _______ atm when the R value is 0.0821. 5. a. b. c. d. 6. a. b. c. What effect will the following changes have on the pressure of a fixed amount of gas? an increase in temperature at constant volume PT a decrease in volume at constant temperature doubling the volume at constant temperature P doubling the temperature and halving the volume What effect will the following changes have on the volumeXof a fixed amount of gas? an increase in pressure at constant temperature a decrease in temperature at constant pressure a decrease in pressure coupled with an increase in temperature. II P2 4 Pl y TV 7. State Dalton’s law of partial pressures in words and in the form of a mathematical equation. Thepressure mixture gases of P of each a of pressure gas to the sum thepartial equal of t Pz Pz is Protal 8. Calculate the new pressure if a 4350 mL of a gas at a pressure of 1.38 atm is allowed to contract to a volume of 2.25 L. PV PzV2 138 atm 4.3504 PzG 25L P2 2.67utm 9. Calculate the new volume if 4.53 L of a gas at 32.0oC is subjected to a drop in temperature of 10.0oC. III ma 10. What mass of oxygen gas occupies 10.0 L if 4.20 g of oxygen under the same conditions occupies 100. L? because n normally is moles but present there is only lgas youcan 19 D.to use grams g 11. A sample of He gas has a pressure of 890 mmHg at a temperature of –54oC. At what pressure (atm) will a sample of helium reach a temperature of 408oC? s E E Ei Pz tg 2800mutts zatmy 12. A 12.0 L sample of gas is emitted 21,000mg from a volcano with a pressure of 1.20 atm and a o temperature of 150.0 C. What is the volume of the gas when its pressure is 684 mmHg and the temperature is -10.0oC? 3 47 It Eve Vz 9g 9 13. What volume does 92.0 g of oxygen gas occupy at 5.20oC and 1525 mmHg? V 488 V YI 92.0g 01 4 11 3270 2.88mA 1525mm Hstommmage2.007dm 68.204 14a. Propane gas (C3H8) burns completely to form carbon dioxide and water. Write a balanced chemical equation. Hst 502 3 302 4420 b. If 14.5 L of O2 and 2.53 L of propane are present in the reaction at STP, how many liters of carbon dioxide are formed at 1.5 atm and 500oC? 14.5202x FL x 22 FIX 2.53LGH8x 1 111 1 V14.30 1 388molCO2 g 3391102 767314 900am 684mm'tsting Liquids and Solids 1. Identify the similarities and differences of solids, liquids, and gases and describe how the kinetic molecular theory helps explain the differences between solids, liquids, and gases. solids liquids sign volume versa proximity 2. really close gases extremelyfarapart close Infinite indefinite List the intermolecular forces from strongest to weakest. definite H bonding dipole dipole Londondispersion forces Themorepolar thestrongerthe force Infinite indefinite Why are they in this order? attractionbetweenmolecules of 3. Name the strongest intermolecular force for the following compounds: H2O CH4 NH3 N2 PBr3 Ne HF SiCl4 Abond LDF fond of ionic nonpolar itbonding LDF 4. Know the following terms: melting point, freezing point, evaporation, condensation, boiling point, sublimation, deposition temperature which phasechangeoccurs MP a s i solid Egg liquid liquid YEEII.onga himation sold Fositiongas bp fp pressure atmosphericpressure boiling whenvapor moleculeson surfacehave evaporation when i.gsliquid tsantim 5. Explain the difference between evaporation and boiling. 6. The melting point of acetone (the main ingredient in nail polish remover) is –95oC and its boiling point is 57oC. Sketch a heating curve for acetone from –105oC to 70oC. Indicate where the boiling points and melting points are and the various states. At what temperature will both liquid and solid be present? temp 57 L g Ltg 7. Draw a phase diagram for water. Indicate where you would find a solid, liquid, and gas. pram Jaffe point 8. Define triple point. Triplepoint is the temperature solid liquid gas pressure are in equilibrium at which all 3 phases 9. Explain viscosity. How does the viscosity of water compare to the viscosity of nonpolar liquids? What can you conclude about the attractive forces between molecules of a highly viscous liquid? Why does the viscosity of liquid increase when the temperature is lowered? nonpolar Ho has a higher viscositythan molecules Viscosity resistance to flow are more attractiveforces between there because liquids harder themtoseparatewhen molesmoveslower for flowing AtlowerT so it is 10a. What equation would be used to calculate the amount of heat used to heat a substance? Cbt M q M DHfus c. Why areq these equations different? Why can’t one equation be used for both? Hint: think about what the heating curve looks like. b. Melt a substance? Whenheating thetemperatureandkineticenergyt potentialenergyT Whenmelting there is notemperature Tandonlythe Solutions 1. What are the factor(s) that increase the rate of dissolution? Ttemperature Tagitation Tsurfacearea 2. What are the factor(s) that increase the solubility of a solid in a liquid? Ttemperature likepolarity dissolveslike 3. What are the factor(s) that increase the solubility of a gas in liquid? Itemperature Tpressure noagitation 4. Given the solubility graph handed out in class, a. What is the solubility of sodium nitrate in 850 mL of water at 80oC? b. What is the solubility of sodium nitrate in 850 mL of water at 25oC? 3 Iggy X 1215.5gNanos Nato X 765g Fogh 9425 1 c. How much sodium nitrate would precipitate from the 850 mL solution that was at 80oC if it was cooled to 25oC? 1215 5g 5. How does a solution form? 765g 450.5 g ppt ionin acrystallattice the sidef The sidef H2O o isattractedtothe it molecule attractsitaway fromthecrystallattice thydrates orsurrounds latticeandhydrates it fromthe The sideofits a isattracted to ion pullsitaway covalent apolar 6. Explain the difference between saturated, unsaturated, and supersaturated solutions. saturated themaximum amt solidis dissolvedyoucanseeit iftheant abovesolubility cure ofdissolved Caltseesolid unsaturated less thanMax is supersaturated morethanmaxisdissolved canseesolid if above curve 7. What is an aqueous solution? A sold dissolved utto 8. What is the molality of a solution that has 68.3 g of copper (II) nitrate dissolved in 1500. g of water? CnCN0312 683g M myth gg 364m ol Assuming VitroVsoh 134 23MI 9. What is the equation for molarity? M mytton 10. What is the molarity formed by mixing 10.0 g H2SO4 with enough water to make 100.0 mL of solution? gg 10.0gttzsoax o.ua t.gg ff 1.02m 125g1tC4 Yxfd 11. Vinegar is a solution of acetic acid. What is the molarity of the solution produced when 125 g of acetic acid (C2H4O2) is dissolved in sufficient water to prepare 1.50 L of solution? 1.39M 12. How many mL of 12 M HCl is needed to make a 0.250 L of 3.5 M solution of HCl? MV 42mLV MzV2 3.5M 250mL V 73mL 13. Predict the products. balance, write the total ionic and net ionic equations. a. ___FeCl2 (aq) + ___NaOH (aq) → 2 2NaCl Felonies Total Ionic: Felt za Net Ionic: Felons s 2Nett204 Fettig FebLcs 204Cag b. ___HCl (aq) + ___Pb(NO3)2 (aq) → 2 Total Ionic: 24 1 2d Net Ionic: 2Nd za PbUse t 2ANDLag Pbdies t 2Ht 2ND Po 2ND Pbclacs Pb capt212g c. ___CuCl 2 (aq) + ___(NH4)3PO4 (aq) → 3 2 Cuz 4126 Total Ionic: 3 Litt 64 6NHytt28043 3 a'cap 2Pa Net Ionic: g p CuzPalas 6NHycleay 6NHyt 64 du6042 s 14. How many grams of silver chromate are formed when 250 mL of 1.5 M silver nitrate reacts with 155 mL of 3.2 M sodium chromate? What is the final molarity of sodium nitrate? B c 2Agnos t NaCroy 250465M 05541312M 375m01 496m01 2x1875mA x Agave42Nanos O X X Ag2604 1875mn 7 1 031 45 53.20gAgarose 926MNanos 3774 Acids and Bases 1. What is the Arrhenius definition of an acid? A base? Acid Base dissolves in H2o to form Ht OH 2. What is the Bronsted-Lowry definition of an acid? A base? Acid Base Ht donor Ht acceptor 3. What is a neutralization reaction? Anacid t basereacttoform a salt water Anndicatorchangescolor w changingpH 4. What is an indicator? List 2 examples. Examples phenolphthalein universal indicator 5. List the 6 strong acids – names and formulas. II HB S hydrobromicacid My redcabbage hydrangeas etc arsonsulfuricacid 6. What do all strong bases have in common (besides the presence of OH-)? Theycompletely dissociatein H2O 7. Complete the following table [H3O+] pH 1 x 10-3 3 9 110 97 1 102 [OH-] 1 10 -5 1 x 10 1 10 7-12 7 2 1 10 1 x 10 8. What is the pH of the following solutions? a. 0.00432 M HCl Ht xEf I 0.169Mott x Iggy 00432mF b. 0.0847 M Ca(OH)2 pOH 11 5 7 12 log00432 p Acidic, basic, or neutral acid base neutral acid 2.365 Potts log769 772 pH 14 772 13.228 c. 0.0053 M acetic acid (10% dissociation) X ten d. 0.052 M Mg(OH)2 (5% dissociation) t204 of 4 PH log5.310 3.28 5.3104 0052M OH ftp.T X2mgg POH log0052 2.28 PH Mg 9. What is the molarity mg of a 10.0 mL sample of sulfuric acid solution that is titrated with14 25.0 mL of 0.50 M NaOH? Colt Has Oyt2NOH 100mL Naz504 t 2h20 38Th I4 0250LNaotxomofy.fi 0063molH so4 2.28 11.72 M not i89E7If35q 10. What is the molarity of a 20.0 mL sample of phosphoric acid solution that is titrated with 16.0 mL of 1.0 M NaOH? Assume that phosphoric acid is a strong acid (even though its really not). HzPoyt3Neolt 053mHz Naoh sNaspoat3tz 160L t.gl It P .o Poy 5 4314 am HzPoy 11. What is a buffer? Explain what a buffer is composed of and how it works. anditsconjugatebase resistschanges inpitmade a weakacid Abufferis a solutionthat of buffer added to it isneutralized the the or a weakbase its conjugateacid If acid is buffer it is neutralized the basiccomponent thebuffer ifbaseis addedto the by by acidiccomponentofthebuffer of 12. A seashell is composed largely of calcium carbonate and is placed in a solution of HCl. As a result, 1500. mL of dry CO2 gas at STP is produced. The other products are CaCl2 and water. a. Write a balanced chemical equation. Ceci t Hel Caco coat420 b. Based on this information, how many grams of CaCO3 are consumed in the reaction? Efx to 1500 coax 3x 919 5.901gCaco c. What volume of 2.00M HCl solution is used in this reaction? 1500 LaxImage fgxIn 0.06696L or66.96mL 13. In a titration, 27.4 mL of 0.0154 M Ba(OH)2 is added to a 20.0 mL sample of HCl solution of unknown concentration. a. Write a balanced chemical equation. 244 Bacon 20.0mL Y Beast2420 MI b. What is the molarity of the acid solution? o 027440.015421Bacotax M my 8 Inol ftgy 0 0422M HCl 8.44mmol Hd c. What is the pH of the acid solution? 0422 Helx mil HI 0422mgHt pH log0422 1.375