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-1- Honors Unit 3 Stoichiometry Homework & Handouts Miss Adams Chemistry 1 Name: ______________________________ -2- Molar Mass Worksheet Calculate the molar masses of the following chemicals: 1) KOH 2) BeCl2 3) BF3 4) Mg(OH)2 5) UF6 6) H3PO4 7) (NH4)2SO4 8) CH3COOH 9) Pb(NO3)2 10) Ga2(SO3)3 -3- Mole Conversions Worksheet Directions: Solve the problems below. Report your answers to the correct number of significant figures and with the correct units. ***Remember: 1 mole = 6.02 x 1023 representative particles = molar mass (grams) 1. Calculate the number of CO2 molecules in 3.00 moles. 2. Calculate the mass in grams of 5.0 moles of Li. 3. Calculate the number of formula units found in 148.0 g of Ca(OH)2. 4. How many atoms of carbon are in a pencil if the mass of carbon is 2.00 g? 5. How many formula units of MgCl2 would have a mass of 345 kg? 6. Calculate the number of ammonium ions in 0.376 moles of ammonium sulfate. 7. How many potassium atoms are in 0.320 moles of potassium phosphate? -4- Empirical & Molecular Formula Problems (pg. 4 & 5) Show work to solve each problem below. Read each question carefully and think about what you need to do to solve the problem. 1. A sample of benzotrifluoride was found to contain 57.54 grams of carbon, 3.4 grams of hydrogen, and 39.10 grams of fluorine after combustion analysis. Determine the empirical formula of the compound. 2. The molar mass of a compound is 92 g/mol. Analysis of a sample of the compound indicates that it contains 0.606 g N and 1.390 g O. Find its empirical and molecular formula. 3. Determine the molecular formula of the compound with an empirical formula of CH and a molar mass of 78.110 g/mol. -54. What’s the empirical and molecular formula of a molecule containing 18.7% lithium, 16.3% carbon, and 65.0% oxygen? The molar mass of the compound is 73.8 g/mol. Name of compound:___________________________________________ 5. If 4.04 g of N combine with 11.46 g O to produce a compound with a molar mass of 108.0 g/mol, what is the empirical & molecular formula of this compound? -6- Writing Chemical Equations (pg. 6 & 7) Use the naming & writing rules from Unit 2 as well as the notation we discussed in this unit to write the following chemical equations. Pay attention to whether a substance is ionic or molecular/covalent when writing the formula! 1. Zinc metal and aqueous lead (II) nitrate react to form aqueous zinc nitrate and solid lead. 2. Aqueous aluminum bromide and chlorine gas react to produce aqueous aluminum chloride and liquid bromine. 3. Aqueous sodium phosphate and aqueous calcium chloride form aqueous sodium chloride and calcium phosphate as a precipitate. 4. Potassium metal and chlorine gas combine to form aqueous potassium chloride. -75. Aluminum metal and aq. hydrochloric acid (hydrogen chloride) react to form aqueous aluminum chloride and hydrogen gas. 6. Aqueous calcium hydroxide and phosphoric acid (hydrogen phosphate) form calcium phosphate as a precipitate and liquid water. 7. Copper metal and sulfuric acid (hydrogen sulfate) yield aqueous copper (II) sulfate, liquid water, and gaseous sulfur dioxide. 8. Hydrogen gas and nitrogen monoxide gas produce gaseous water and nitrogen gas. -8- Balancing Chemical Equations Place the correct coefficients on the lines to balance the equations below: 1) ____ N2 + ____ H2 ____ NH3 2) ____ KClO3 ____ KCl + ____ O2 3) ____ NaCl + ____ F2 ____ NaF + ____ Cl2 4) ____ H2 + ____ O2 ____ H2O 5) ____ Pb(OH)2 + ____ HCl ____ H2O + ____ PbCl2 6) ____ AlBr3 + ____ K2SO4 ____ KBr + ____ Al2(SO4)3 7) ____ CH4 + ____ O2 ____ CO2 + ____ H2O 8) ____ C3H8 + ____ O2 ____ CO2 + ____ H2O 9) ____ C8H18 + ____ O2 ____ CO2 + ____ H2O 10) ____ FeCl3 + ____ NaOH ____ Fe(OH)3 + ____NaCl 11) ____ P + ____O2 ____P2O5 12) ____ Na + ____ H2O ____ NaOH + ____H2 13) ____ Ag2O ____ Ag + ____O2 14) ____ S8 + ____O2 ____ SO3 15) ____ CO2 + ____ H2O ____ C6H12O6 + ____O2 16) ____ K + ____ MgBr ____ KBr + ____ Mg 17) ____ HCl + ____ CaCO3 ____ CaCl2 + ____H2O + ____ CO2 18) ____ HNO3 + ____ NaHCO3 ____ NaNO3 + ____ H2O + ____ CO2 19) ____ H2O + ____ O2 ____ H2O2 20) ____ NaBr + ____ CaF2 ____ NaF + ____ CaBr2 21) ____ H2SO4 + ____ NaNO2 ____ HNO2 + ____ Na2SO4 © 2000 Cavalcade Publishing – All Rights Reserved For chemistry help, visit http://www.chemfiesta.com -9Balancing Chemical Equations Worksheet Directions: Place the correct coefficients on the lines in order to balance the following equations. 1) ____ Na3PO4 + ____ KOH ____ NaOH + ____ K3PO4 2) ____ MgF2 + ____ Li2CO3 ____ MgCO3 + ____ LiF 3) ____ P4 + ____ O2 ____ P2O3 4) ____ RbNO3 + ____ BeF2 ____ Be(NO3)2 + ____ RbF 5) ____ AgNO3 + ____ Cu ____ Cu(NO3)2 + ____ Ag 6) ____ CF4 + ____ Br2 ____ CBr4 + ____ F2 7) ____ HCN + ____ CuSO4 ____ H2SO4 + ____ Cu(CN)2 8) ____ GaF3 + ____ Cs ____ CsF + ____ Ga 9) ____ BaS + ____ PtF2 ____ BaF2 + ____ PtS 10) ____ N2 + ____ H2 ____ NH3 11) ____ NaF + ____ Br2 ____ NaBr + ____ F2 12) ____ Pb(OH)2 + ____ HCl ____ H2O + ____ PbCl2 13) ____ AlBr3 + ____ K2SO4 ____ KBr + ____ Al2(SO4)3 14) ____ CH4 + ____ O2 ____ CO2 + ____ H2O 15) ____ Na3PO4 + ____ CaCl2 ____ NaCl + ____ Ca3(PO4)2 16) ____ K + ____ Cl2 ____ KCl 17) ____ Al + ____ HCl ____ H2 + ____ AlCl3 18) ____ N2 + ____ F2 ____ NF3 19) ____ SO2 + ____ Li2Se ____ SSe2 + ____ Li2O 20) ____ NH3 + ____ H2SO4 ____ (NH4)2SO4 - 10 Balancing Chemical Equations Worksheet Directions: Place the correct coefficients in front of the formulas in order to balance the following equations. 1. _____ CaO + _____ P2O5 _____ Ca3(PO4)2 2. _____ Ca3(PO4)2 + _____ H2SO4 _____ CaSO4 + _____ H3PO4 3. _____ NaHCO3 + _____ H2SO4 _____ Na2SO4 + _____ H2O + _____ CO2 4. _____ H2S + _____ Cl2 _____ S8 + _____ HCl 5. _____ Fe(OH)3 _____ Fe2O3 + _____ H2O 6. _____ H3BO3 _____ H4B6O11 + _____ H2O 7. _____ C8H16 + _____ O2 _____ CO2 + _____ H2O 8. _____ Na4P2O7 + _____ Al2(SO4)3 _____ Al4(P2O7)3 + Na2SO4 9. _____ K2CO3 + _____ H3PO4 _____ K3PO4 + _____ H2O + _____ CO2 10. _____ Al4C3 + _____ H2O _____ CH4 + _____ Al(OH)3 - 11 - Writing Word Equations Directions: Write a balanced symbolic equation from the following word equations and classify the type of reaction. 1. iron + sulfur iron (II) sulfide Type:____________________ 2. magnesium chloride + silver nitrate magnesium nitrate + silver chloride Type:____________________ 3. Calcium oxide + water calcium hydroxide Type:___________________ 4. Magnesium bromide + chlorine magnesium chloride + bromine Type:____________________ 5. butane (C4H10) + oxygen carbon dioxide + water Type:__________________ 6. copper (II) nitrate copper (II) oxide + nitrogen dioxide + oxygen Type:____________________ 7. potassium chloride + lead (II) nitrate lead(II) chloride + potassium nitrate Type:____________________ - 12 - Predicting Products Directions: Predict the product(s) for each reaction. Next, write a balanced symbolic equation. 1. magnesium + oxygen 2. sodium chromate + silver nitrate 3. hydrogen peroxide 4. Magnesium + iron (III) bromide 5. heptene (C7H14) + oxygen 6. copper (II) sulfate + barium hydroxide 7. sodium iodide + lead (II) nitrate 8. zinc + copper (II) sulfate - 13 - - 14 - Limiting Reactants (pg. 14 & 15) Show ALL of your work for credit on this assignment! 1. _____ CaO(s) + _____ H2O(l) _____ Ca(OH)2(aq) How many grams of calcium hydroxide will be formed in this reaction when 4.44 g of calcium oxide and 7.77 g of water are available to react? Also identify the limiting reactant. 2. Magnesium undergoes a single replacement reaction with hydrochloric acid. Balanced Equation: How many grams of hydrogen gas will be produced from the reaction of 3.00 g of magnesium with 4.00 g of hydrochloric acid? Identify the limiting reactant. - 15 3. Sulfur reacts with oxygen to produce sulfur trioxide gas. Balanced Equation: If 6.3 g of sulfur reacts with 10.0 g of oxygen, what is the limiting reactant? How many grams of sulfur trioxide will be produced? If 7.01g is actually produced what is the percent yield?