ࡱ> uwt_ |bjbj Wbb8vvd444T8d42wwwJ1L1L1L1L1L1L1$A46p1[ww[[p1E2+++[nJ1+[J1++P.@0P,i^u^.61[202 /67'|7,@0@0n70w"+wwwp1p1www2[[[[7wwwwwwwwwv : Acids, Bases, and Salts Name______________ An Arrhenius acid is defined as any compound that dissociates in aqueous solution to form ____________ ions. HNO3( H+ + NO3 HCl (aq) ( ________________________ An Arrhenius base is defined as any compound that dissociates in aqueous solution to form ____________ ions. KOH (aq)( K+ (aq) + OH- (aq) NaOH (aq)( ________________________ Salts are compounds that dissociate in aqueous solution releasing neither ____________ ions nor ____________ ions. KCl (aq) ( K+ (aq) + Cl- (aq) NaCl (aq) ( ________________________ Using the Arrhenius definition, classify the following examples as acids, bases, or salts: HBr ____________________ KCl __________________ Mg(OH)2 ________________ H3PO4 ________________ HCl ____________________ HClO _________________ KNO2 ___________________ Al(OH)3 ________________ HFO4 ___________________ KC2H3O2 _______________ Ba(OH)2 _________________ NaCl __________________ Acids and bases can also be identified using an operational definition. Operational definitions are simply a list of properties. ACIDS: f& A ____________ taste is a characteristic property of all acids in aqueous solution. f& Acids react with some metals to produce ____________ gas. f& Because aqueous acid solutions conduct electricity, they are identified as ____________. f& Acids react with bases to produce a ____________ and water. f& Acids turn ____________ different colors. BASES: f& Bases tend to taste ____________ and feel ____________. f& Like acids, aqueous basic solutions conduct ____________, and are identified as ____________. f& Bases react with ____________ to produce a salt and ____________. f& Bases turn ____________ different colors. Naming Acids Binary acids consist of ____________ elements, the first being ____________. Ternary acids consist of ____________ elements. Do NOT use a prefix. ate becomes _______ and ite becomes _______ Give the word equation for the neutralization reaction of an acid and a base. Chemical Quantities Worksheet Name ______________________________ Period _____ Date ___________________ Recipes often specify the number of eggs needed. Although eggs are used individually when cooking small quantities, they are sold by the dozen, or by the gross (144, a dozen dozens), depending on the quantity wanted. If you were cooking for an army, you'd likely mix your eggs by the gross, rather than counting them individually. Instead of thinking in terms of 2 eggs per potato, you'd use 2 gross of eggs per gross of potatoes. If you were buying rice for a casserole, would you go to a store and ask for 250,000 rice grains? Or would you ask for a pound of rice? Because rice is small, it's convenient to use other means of measuring than counting. Chemical particles (atoms, molecules, etc.) are much, much, smaller than eggs or rice. It is therefore more convenient and useful to specify quantities in ways other than by counting individual atoms or molecules. The quantity called the mole is used to specify the number of particles, just like the dozen or gross is used for eggs and other items we encounter in our daily lives. Whereas a dozen is 12 of something, and a gross is 144 of something, a mole is 6.02 x 1023 of something (602,000,000,000,000,000,000,000). If a chemical reaction involves one atom of magnesium and two units of hydrochloric acid, one mole of magnesium will react with two moles of hydrochloric acid. We can't pick out individual chemical particles, but we can easily measure a mole of them. How do we measure moles? We use a balance to determine the mass, and then convert mass to moles. Just as the mass of a gross of eggs differs from the mass of a gross of potatoes, the mass of a mole of aluminum atoms differs from the mass of a mole of calcium. The periodic table tells us the mass of one mole of each element. For instance, a mole of aluminum has a mass of 26.98 grams. A mole of calcium has a mass of 40.08 grams. Use the periodic table to determine the mass of the following quantities of chemical substances. Remember, the periodic table tells you the MOLAR MASS, the mass of one mole of each element. The mass of two moles would be twice that of one mole. For compounds, add the molar masses in the ratios indicated in the chemical formulas for the molar mass of the compound. 1 mole of lithium _______________ 1 mole of magnesium _______________ 1 mole of carbon _______________ 1 mole of oxygen _______________ 2 moles of oxygen _______________ 1 mole of hydrogen _______________ 2 moles of hydrogen _______________ 1 mole of H2O _______________ 1 mole of CO2 _______________ 2 moles of CO2 _______________ Use the periodic table to determine the number of moles in the following masses. Remember, the periodic table tells you the MOLAR MASS, the mass of one mole of each element. For compounds, add the molar masses in the ratios indicated in the chemical formulas for the mass of one MOLE of the COMPOUND. Divide the mass indicated by the molar mass to calculate the number of moles. 35.45 grams of chlorine _______________ 63.55 grams of copper _______________ 18.024 g of beryllium _______________ 36.033 grams of carbon _______________ 100 grams of hydrogen _______________ 100 grams of iron _______________ 100 grams of lead _______________ 18.0 grams of H2O _______________ 36.0 grams of H2O _______________ 100 grams of H2O _______________ 1. Balance the following equation: ____ K2PtCl4 + ___ NH3 ! ___ Pt(NH3)2Cl2 +___ KCl Determine the grams of KCl produced (theoretical yield) if you start with 34.5 grams of NH3. 2. Balance the following equation: H3PO4 + 3 KOH ! K3PO4 + 3 H2O If 49.0 g of H3PO4 reacts, how many grams of K3PO4 should be produced? 3. Balance the following equation: Al2(SO3)3 + 6 NaOH ! 3 Na2SO3 + 2 Al(OH)3 If you start with 389.4 g of Al2(SO3)3 and how many grams of Na2SO3 would be produced? 4. Balance the following equation: Al(OH)3 (s) + 3 HCl (aq) ! AlCl3 (aq) + 3 H2O (l) If you start with 50.3 g of Al(OH)3 how many grams of AlCl3 would you expect to produce? Assume you did the experiment and you only got 39.5 g of AlCl3, what is the percent yield (hint: think about how you determine your % for a test what you got divided by what you should have gotten)? 5. Balance the following equation: K2CO3 + 2 HCl ! H2O + CO2 + 2 KCl Determine the theoretical yield (grams) of H2O if you start with 34.5 g of K2CO3. If only 3.4 g of H2O is produced, what is the percent yield? Balance the following equation: H2SO4 + Ba(OH)2 ! BaSO4 + 2 H2O If 98.0 g of H2SO4 reacts, how many grams of BaSO4 should be produced? b) What is the percent yield if you only produce 213.7 g of BaSO4? (use the answer from a to determine the answer for b) Gas Laws SHOW ALL WORK FOR ALL PROBLEMS I. 1.0 atm = 101.3 kPa = 760 mmHg And 0(C = 273 K Change the following units: 359 kPa = _________ atm 10(C = ________ K 6.2 atm = ________ kPa 10K = _______ (C For the rest of the problems: First identify each number with P, V, or T. Second state whose law you are using, Third show the equation, Fourth solve the problem, and Fifth - circle your final answer - and make sure you don't forget your units!!! The gas in a sealed can is at a pressure of 3.00 atm at 25(C. A warning on the can tells the user not to store the can in a place where the temperature will exceed 52(C. What would the gas pressure in the can be at 52(C? A sample of hydrogen exerts a pressure of 0.329 atm at 47(C. The gas is heated 77(C at constant volume. What will its new pressure be? 3. A sample of neon gas occupies a volume of 752 mL at 25(C. What volume will the gas occupy at standard temperature if the pressure remains constant? A sample of oxygen gas has a volume of 150 mL when its pressure is 440 mmHg. If the pressure is increased to standard pressure and the temperature remains constant, what will the new gas volume be? Ral3ph had a helium balloon with a volume of 4.88 liters at 150 kPa of pressure. If the volume is changed to 3.15 liters, what would be the new pressure in atm? 6. 5.36 liters of nitrogen gas are at -25(C and 733 mm Hg. What would be the volume at 128(C and 1.5atm? 7. At constant temperature, 2 L of a gas at 4 atm of pressure is expanded to 6 L. What is the new pressure? (Do this one conceptually and not algebraically.) Thermochemistry Specific Heat Worksheet C = q/m"T, where q = heat energy, m = mass, and T = temperature Remember, "T = (Tfinal  Tinitial). Show all work and proper units. 1. A 15.75-g piece of iron absorbs 1086.75 joules of heat energy, and its temperature changes from 25C to 175C. Calculate the specific heat capacity of iron. 2. How many joules of heat are needed to raise the temperature of 10.0 g of aluminum from 22C to 55C, if the specific heat of aluminum is 0.90 J/gC? 3. To what temperature will a 50.0 g piece of glass raise if it absorbs 5275 joules of heat and its specific heat capacity is 0.50 J/gC? The initial temperature of the glass is 20.0C. 4. Calculate the heat capacity of a piece of wood if 1500.0 g of the wood absorbs 6.75104 joules of heat, and its temperature changes from 32C to 57C. 5. 100.0 mL of 4.0C water is heated until its temperature is 37C. If the specific heat of water is 4.18 J/gC, calculate the amount of heat energy needed to cause this rise in temperature. What is enthalpy? What is enthalpy? What is Hesss Law? Find theHfor the reaction below, given the following reactions and subsequentHvalues: PCl5(g) ! PCl3(g) + Cl2(g) P4(s) + 6Cl2(g) ! 4PCl3(g)H= -2439 kJ 4PCl5(g) ! P4(s) + 10Cl2(g)H= 3438 kJ (2) Find theHfor the reaction below, given the following reactions and subsequentHvalues: 2CO2(g) + H2O(g) ! C2H2(g) + 5/2O2(g) C2H2(g) + 2H2(g) ! C2H6(g)H =-94.5 kJ H2O(g) ! H2(g) + 1/2O2(g)H =71.2 kJ C2H6(g) + 7/2O2(g) ! 2CO2(g) + 3H2O(g)H =-283 kJ 3) Find theHfor the reaction below, given the following reactions and subsequentHvalues: N2H4(l) + H2(g) ! 2NH3(g) N2H4(l) + CH4O(l) ! CH2O(g) + N2(g) + 3H2(g)H= -37 kJ N2(g) + 3H2(g) ! 2NH3(g)H= -46 kJ CH4O(l) ! CH2O(g) + H2(g)H= -65 kJ (4) Find theHfor the reaction below, given the following reactions and subsequentHvalues: H2SO4(l) ! SO3(g) + H2O(g) H2S(g) + 2O2(g) ! H2SO4(l)H= -235.5 kJ H2S(g) + 2O2(g) ! SO3(g) + H2O(l) H= -207 kJ H2O(l) ! H2O(g).< D E Y b c    > R \      $ % 2 5 : ; A B ɷɷɣɕɕɣɕڕɕɕɃɕɃɃɕɕɕɕɃɕɕɃ#h^h^CJH*OJQJ^JaJh^CJOJQJ^JaJ& jh^h^CJOJQJ^JaJ#hgh^CJH*OJQJ^JaJ h^h^CJOJQJ^JaJ#h^h^CJOJQJ\^JaJ&hh^5CJOJQJ\^JaJ3-.< Y }  3 4 ! 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What is nuclear Fusion? Where is Nuclear Fusion used? What are Isotopes? What is a chain reaction? Write the equations for: the alpha decay of radon198 2) The beta decay of uranium 237 3) Positron emission from sodium 22 4) Write the symbols for an alpha particle, beta particle, gamma ray, and positron. 5) If the half-life for the radioactive decay of Mendelevium 101 is 5 minutes and I start with a 130 gram sample, how much will be left over after 60 minutes? Chemistry Semester Two Key Term List These are the terms you are expected to know the meaning of when read, by the time you have completed Spring Chemistry. Molarity solute Solvent boiling point elevation Brownian motion colligative property concentration dilution freezing point depression heat of solution hydrogen bonding immiscible insoluble miscible osmotic pressure osmosis saturated solubility solution supersaturated unsaturated amphoteric neutralization Acid Anhydride Arrhenius acid/base Base Bronsted-Lowry model buffer conjugate acid/base equivalence point Hydronium ion Indicator Ionization pH, pOH salt standard solution strong acid/base titration weak acid/base Ka and Kb Lewis acid/base Kelvin Standard pressure Standard temperature atmospheric pressure Avogadro s principle Barometer Boyle s Law Charles s Law Combined Gas Law Gay-Lussac s Law Ideal Gas Law Kinetic molecular theory Pascal enthalpy specific heat activated complex activation energy calorie catalyst collision theory energy entropy heat heat of formation heat of reaction inhibitor intermediate Joule law of conservation of energy reaction rate spontaneous process thermochemical equation chemical potential energy Gibbs Free Energy spontaneous reaction state functions fission fusion alpha particle atom atomic mass atomic mass unit atomic number beta particle chain reaction electron gamma radiation half-life isotope mass number neutron nuclear reaction nucleus positron proton radiation radioactive decay Functional group Organic molecule Alcohols Aldehydes Alkane Alkene Alkyl Halides Alkyne Amines Aromatic Carboxylic acids Cycloalkanes Esters Ethers Geometric isomers Ketones Monomer Polymer Saturated hydrocarbons Structural isomers Unsaturated hydrocarbon     Spring 2-14 Chemistry Review Material Answer questions and problems on your own paper. 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