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Unit 3 IB Topic 1 Quantitative Chemistry Unit Vocabulary: Elements: Atoms: Compounds Molecule: Mole: Ar: Mr: N: n (g mol-­‐1): Avogado’s Constant (L): Molecular Formula: Empirical Formula: Kinetic energy: Potentials energy: Evaporation: Condensation: Sublimation: Intermolecular Forces: Hydrogen Bonding: Dipole-­‐dipole: van der Waals force (London Dispersions): Chemical equation: Reactants: Product: Coefficients: Limiting reactant: Experimental yield: Theoretical yield: Percentage yield: Avogadro’s hypothesis: Molar volume: Solution: Solvent: Solute: Aqueous (aq): Titration: Mole Problems Determine the number of moles found in 24 grams of carbon? A lab requires 43 moles of Sulfur. How many gram must the chemist mass? The 65 grams of chlorine (Cl2) was produced during a chemical reaction. How many moles are in the chlorine? A combustion reaction produces 234 grams of water (H2O). How many mole of water are in the sample? A chemist needs 34.5 mole of hydrochloric acid (HCl). How many grams are required? A recipe requires 24 grams of salt (NaCl). How many mole does the 24 grams contain? Determine the number of molecules in a 2 moles of H2O. 3.5 mole of nitrogen gas (N2) contains how many molecules? 45.6 grams of water contains how many molecules of water? Determining Empirical and molecular formulas A. Calculate the percent composition for the following compounds.
1. Cr2O3
2. Ca3(PO4)2
B. Calculate the percent by mass of iron in each of the following compounds.
3. iron (III) oxide
4. iron (II) oxide
C. Determine the empirical formula for each compound.
5.
A compound contains 0.0130 mol carbon, 0.0390 mol hydrogen, and 0.0065 mol oxygen.
6.
A compound consists of 72.2% magnesium and 27.8% nitrogen by mass.
7.
Glucose contains 40.0% carbon, 6.7% hydrogen, and 53.3% oxygen by mass.
8. Phosphoric acid is found in some soft drinks. A sample of phosphoric acid contains 0.3086 g of hydrogen,
3.161 g of phosphorus, and 6.531 g of oxygen.
D. Determine the molecular formula for each compound described.
9. A compound has an empirical formula of NO2 and a molar mass of 92.02 g/mol.
10. A compound has an empirical formula of C2H3O and a molar mass of 172 g/mol.
11. Ibuprofen, a common headache remedy, has an empirical formula of C7H9O and a molar mass of
approximately 215 g/mol.
12. Nicotine is 74.1% carbon, 8.6% hydrogen, and 17.3% nitrogen by mass. Its molar mass is about 160 g/mol.
13. Epinephrine (adrenaline) is a hormone secreted into the bloodstream in times of danger and stress. It is 59.0%
carbon, 7.1% hydrogen, 26.2% oxygen, and 7.7% nitrogen by mass. Its molar mass is about 180 g/mol.
E. Questions
14. Can the molecular formula of a compound ever be the same as the empirical formula?
Explain your answer.
15. What is the empirical formula of a compound that has three times as many hydrogen atoms as carbon atoms,
but only half as many oxygen atoms as carbon atoms?
States of Matter: Procedure: • Open the internet browser and enter the address: http://phet.colorado.edu • Click on “Play with Sims” and select “Chemistry” from the menu on the left. • Open the “States of Matter” Simulation and select “Run Now” Investigation: 1. Predict what the molecules of a solid, liquid and gas look like. Illustrate your prediction with a drawing. Solid Liquid Gas 1a. Predict how a change in temperature (heat or cold) will effect each phase change. 1. complete the table below by exploring the “Solid, Liquid, Gas” tab in the simulation. Test your predictions and record your observations by recording the temperature and illustrations of each substance in the three states of matter. Substances Neon Argon Oxygen Water Observations Solid Temperature: Illustration: Temperature: Illustration: Temperature: Illustration: Temperature: Illustration: Liquid Temperature: Illustration: Temperature: Illustration: Gas Temperature: Illustration: Temperature: Illustration: Temperature: Illustration: Temperature: Illustration: Temperature: Illustration: Temperature: Illustration: 2. Interpret the graph of Kinetic Energy vs. Temperature. Using the graph describe the relationship between Kinetic Energy and Temperature. Temperatu
re Celsius Gas qu
idi
d S
o
li
Energy d 3. Write a conclusion, using the simulation and graph. Use what you have learned in this activity to support the following two statements. • How the molecules in a solid, liquid and gas compare to each other. • How temperature relates to the kinetic energy of molecules. Balance and state the type for these equations: 1. _____Ca(OH)2(s) + _____HCl(aq) -­‐-­‐-­‐> ____CaCl2(aq) + _____H2O(l) 2. _____FeCl3(aq) + _____(NH4)2S(aq) -­‐-­‐-­‐> _____Fe2S3(s) + _____NH4Cl(aq) 3. _____KNO3 (s) -­‐-­‐-­‐> _____KNO2 (s) + _____O2(g) 4. _____Ag2O(s) -­‐-­‐-­‐> _____Ag(s) + _____O2(g) 5. _____C4H10(g) + _____O2(g) -­‐-­‐-­‐> _____CO2(g) + _____H2O(g) 6. _____Br2(aq) + _____KI(aq) -­‐-­‐-­‐> _____I2(aq) + _____KBr(aq) 7. _____AsCl3(aq) + _____H2S (aq) -­‐-­‐-­‐> _____As2S3 (s) + _____HCl 8. _____C5H12O (l) + _____O2(g) -­‐-­‐> ______CO2(g) + _____H2O (g) 9. _____Al(s) + _____H2SO4 (aq) -­‐-­‐-­‐> _____Al2(SO4)3(aq) + _____H2(g) 10. _____Fe(s) + _____Cl2(g) -­‐-­‐-­‐> _____FeCl3(s) 11. C5H12 + O2 -­‐-­‐-­‐-­‐-­‐> CO2 + H2O 12. NH3 + O2 -­‐-­‐-­‐-­‐-­‐> N2 + H2O 13. KOH + H2SO4 -­‐-­‐-­‐-­‐-­‐> K2SO4 + H2O 14. N2H4 + N2O4 -­‐-­‐-­‐-­‐-­‐> N2 + H2O 15. F2 + H2O -­‐-­‐-­‐-­‐-­‐> HF + O2 16. Na2O + H2O -­‐-­‐-­‐-­‐-­‐> NaOH 17. Na2CO3 + HNO3 -­‐-­‐-­‐-­‐-­‐> H2O + CO2 + NaNO3 18. Ca3P2 + H2O -­‐-­‐-­‐-­‐-­‐> PH3 + Ca(OH)2 19. IBr + NH3 -­‐-­‐-­‐-­‐-­‐> NI3 + NH4Br 20. NH4NO3 -­‐-­‐-­‐-­‐-­‐> N2 + H2O + O2 Stoichiometry Problems: Given the following equation:
C4H10 + O2 -------> CO2 + H2O, show what the
following molar ratios should be. Mole A to Mole B: Given the following equation:
KClO3 --------> KCl + O2 How many moles of O2 can be produced
by letting 12.00 moles of KClO3 react? Given the following equation:
Cu + AgNO3 ------> Cu(NO3)2 + Ag How many moles of Cu are
needed to react with 3.50 moles of AgNO3?
If 89.5 grams of Ag were produced, how many grams of Cu reacted?
Given the reaction:
NH3(g) + O2(g)---> NO(g)+ H2O(l)
number of moles of products formed is
Mole A to Mass of B or Mass of A to Moles of B: Given the following equation:
NaClO3 ---> NaCl +
When1.20 mole of ammonia reacts, the total
O2
12.00 moles of NaClO3 will produce how many grams of O2?
How many grams of NaCl are produced when 80.0 grams of O2 are also produced?
Mass A to Mass B: Molten iron and carbon monoxide are produced in a blast furnace by the reaction of iron(III) oxide and coke
(pure carbon). If 25.0 kilograms of pure Fe2O3 is used, how many kilograms of iron can be produced? The
reaction is: Fe2O3
+
C
---> Fe +
CO
The average human requires 120.0 grams of glucose (C6H12O6) per day. How many grams of CO2 (in the
photosynthesis reaction) are required for this amount of glucose? The photosynthetic reaction is:
CO2 +
H2O ---> C6H12O6 +
O2
Given the following equation:
Na2O + H2O -------> NaOH How many grams of NaOH is produced from
2
1.20 x 10 grams of Na2O? How many grams of Na2O are required to
produce 1.60 x 102 grams of NaOH?
Percentage Yields: Calculate the percent yields in each of the following cases: a. Theoretical yield 50.0 g of product; actual yield 41.9 g b. Theoretical yield is 290 kg of product; actual yield is 270 kg c. Theoretical yield is 64 kg of product; actual yield is 324 g 1) Chlorobenzene, C6H5Cl, is used in the production of chemicals such as aspirin and dyes. One way that chlorobenzene is prepared is by reacting benzene, C6H6, with chlorine gas according to the following BALANCED equation. C6H6 (l) + Cl2 (g) ! C6H5Cl (s) + HCl (g) a. What is the theoretical yield if 45.6 g of benzene react? b. If the actual yield is 63.7 g of chlorobenzene, calculate the percent yield. 2. When carbon disulfide burns in the presence of oxygen, sulfur dioxide and carbon dioxide are produced according to the following equation. CS2 (l) + 3O2 (g)!CO2 (g) + 2SO2 (g) a. What is the percent yield of sulfur dioxide if the burning of 25.0g of carbon disulfide produces 40.5 g of sulfur dioxide? b. What is the percent yield of carbon dioxide if 2.5 mol of oxygen react and 32.4 g of carbon dioxide are produced? Limiting Reactant: 1) Chlorine can replace bromine in bromide compounds forming a chloride compound and elemental bromine. The following equation is an example of this reaction. KBr + Cl2 -­‐-­‐-­‐-­‐ KCl + Br2 When 0.855 mole of Cl2 and 3.305 g of KBr are mixed in solution, which is the limiting reactant? How many grams of Br2 are formed? 2) AgNO3 + Ni -­‐-­‐-­‐-­‐ Ag + Ni(NO3)2 When 3.3 moles of Ni react with 159.3 grams of AgNO3, which is the limiting and which is the excess reactant? Gas Stoichiometry 1) Calcium carbonate decomposes at high temperatures to form carbon dioxide and calcium oxide: CaCO3(s)  CO2(g) + CaO(s) How many grams of calcium carbonate will I need to form 3.45 liters of carbon dioxide? 2) Ethylene burns in oxygen to form carbon dioxide and water vapor: C2H4(g) + 3 O2(g)  2 CO2(g) + 2 H2O(g) How many liters of water can be formed if 1.25 liters of ethylene are consumed in this reaction? 3) When chlorine is added to acetylene, 1,1,2,2-­‐tetrachloroethane is formed: 2 Cl2(g) + C2H2(g)  C2H2Cl4(l) How many liters of chlorine will be needed to make 75.0 grams of C2H2Cl4?