1 / 30

Stoichiometry: Measurement of Elements

Stoichiometry: Measurement of Elements. Formula Weights. Sum of the atomic weights (amu) of each atom in a chemical formula. Called “ molecular weight ” or “ molecular mass ” for a molecule. Use “ formula weight ” for ionic cmpds. The Mole.

hiroko
Download Presentation

Stoichiometry: Measurement of Elements

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Stoichiometry: Measurement of Elements

  2. Formula Weights • Sum of the atomic weights (amu) of each atom in a chemical formula. • Called “molecular weight” or “molecular mass” for a molecule. • Use “formula weight” for ionic cmpds.

  3. The Mole • Chemists have derived a special counting unit for describing very large numbers of atoms or molecules. • Mole (mol) = the amount of matter that contains as many objects as the number of atoms in exactly 12g of isotopically pure carbon-12.

  4. Mole, cont. • Avogadro’s number: 6.022 x 10^23 • A mole of ANYTHING contains 6.022 x 10^23 objects! • I mole of marbles would cover the entire surface of the earth in a layer ________ thick. • Pennies placed side to side in a straight line would encircle the earth ________ times.

  5. Representative Particles • Species present in a substance.

  6. Moles, cont., cont. • Remember: • 1 mol of carbon = 6.022 X 10^23 atoms. • 1 molwater = ____ molecules. • 1 mol CN-ions = _____ ions. • 1 molNaCl = ____ formula units (f.u.’s). • 1 molelephants = _____ elephants.

  7. Mole-Particle/Particle-Mole Problems • Use dimensional analysis! • How many moles of magnesium are 1.25 x 10^24 atoms of magnesium? • How many moles are 2.80 x 10^24 atoms Si? • How many molecules are in 3.60 mol water? • How many hydrogen atoms are in 3.60 mol water????

  8. Molar Mass • A mole is always the same number but moles of different substances have different masses. • 1 mol water = 18.02 g; 1 mol lead = 207.2 g • Molar mass: the mass in grams of 1 mole of a substance. Unit is g/mol.

  9. Calculating Molar Mass • Calculate molar mass of CH4. • C: 1 atom x 12.01 g/mol = 12.01 g/mol • H: 4 atoms X 1.01 g/mol = 4.04 g/mol • Add together: • 12.01g/mol + 4.04 g/mol = 16.05 g/mol Watch your sig figs!!!

  10. Practice Calculating Molar Mass • Calculate the molar mass of NaCl. • Calculate the molar mass of calcium hydroxide. • Calculate the molar mass of Sr3(PO4)2. • Do you like this more than nomenclature?

  11. Mass-Mole/ Mole-Mass Problems • Use dimensional analysis! • Find the mass of 4.52 x 10^-3 mol water. • Find the mass of 0.342 mol nitrogen gas. • How many moles are in 72.96 g LiCl? • How many moles are in 12 28 g KOH? • Are we having fun yet?

  12. Mole-Volume Relationship • Avogadro’s Hypothesis: equal volumes of gases at the same temp and pressure contain an equal number of particles. • Note: the size or mass of gas particles does NOT matter because particles are so far apart from each other.

  13. Molar Volume of a Gas • STP = standard temp and pressure • Standard temp for gases = 0°C • Standard pressure = 1 atm • “Molar volume of a gas” means that at STP… I mole of ANY gas = 22.4L of gas

  14. Mole-Volume Problems • We use molar volume to do mole-volume problems! Yeah! • Calculate the volume of 3.20 x 10^-3 mol carbon dioxide at STP. • 0.0717 L carbon dioxide • Calculate the volume of 3.70 mol nitrogen gas at STP. • 82.9 L nitrogen gas

  15. More Molar Volume Calculations! • You have 0.200 L hydrogen gas at STP. How many moles? • 8.93 x 10^-3 mol • Dan has 0.375 mol of oxygen gas at STP. What is its volume? • 8.40 L oxygen

  16. Density & Molar Volume at STP • The density of gases is in g/L, NOT g/mL. WHY? • You can use density along with molar volume to get molar mass! Hurrah!

  17. Density & Molar Volume Problems • A gas has a density of 3.58 g/L at STP. What is the molar mass of the gas? • 80.2 g/mol • A gas has a density of 1.964 g/L at STP. What is its molar mass? • 43.99 g/mol • What is the density of krypton gas at STP? • 3.74 g/L

  18. Percentage Composition from Chemical Formula • Percentage by mass of each element in a substance. • % element = (# of atoms x molar mass of element/ molar mass of compound) x 100 • Total % of each element = 100%

  19. Calculating Percentage Composition • Calculate the % composition of C6H12O6. • % C = (6 x 12.01 g/mol/180.2 g/mol) x 100 = 40.00% % H = (12 X 1.01 g/mol/180.2 g/mol) x 100 = 6.73% % O = 100.00% - 40.00% - 6.73% = 53.27%

  20. Percent Composition Practice • Calculate the percent composition of C3H8. • C: 81.8 %; H: 18.2 % • Calculate the percent on nitrogen in NH3. • 82.4% nitrogen

  21. Percent Composition from Mass Data • Percent Composition = (mass of element in cmpd/mass of cmpd) x 100 • Total %’s of all elements in cmpd = 100%

  22. Percent Composition by Mass Practice • When a 13.60-g sample of a cmpd containing only Mg and O is decomposed, 5.40 g oxygen is obtained. What is the percent comp of the cmpd? • O: (5.40 g O/ 13.60 g) x 100 = 39.7% • Mg: [(13.60 g- 5.40 g)/ 13.60 g] x 100 = 60.3%

  23. More Percent Composition Practice • Calculate the number of grams of sulfur in 3.54 g H2S. • First, find the % of sulfur in H2S. • 94.1% S • Then, multiply .941 X 3.54 g H2S. • 3.33 g

  24. Empirical & Molecular Formulas • Empirical formula: gives the lowest whole number ratio of atoms in a compound. PbO, not Pb2O2 • Molecular formula: whole number multiples of the empirical formula.

  25. Determining Empirical Formulas • Sing the Empirical Formula Song (sung to tune of “Twinkle, Twinkle Little Star”): • “Percent to mass, mass to mole, divide by small, multiply ‘til whole.”

  26. Empirical Formula Practice • A compound is analyzed and found to contain 25.9% nitrogen and 74.1% oxygen. What is the empirical formula of the compound? • N2O5

  27. More Empirical Formula Calculations! • Find the empirical formula for the following cmpd: Hg: 67.6%; S: 10.8%; O: 21.6% • HgSO4 • Find the empirical formula for the following cmpd: H: 5.9%; O: 94.1% • HO

  28. Molecular Formulas • Once you have determined the empirical formula (e.f.), you can determine the molecular formula (m.f.) if you know the compound’s molar mass. • Divide the molar mass of the cmpd by the molar mass of the e.f. and get a whole number. Multiply this number by each subscript in the e.f. to get the m.f..

  29. Finding a Molecular Formula • You have the empirical formula HO. Find the molecular formula if its molar mass is 34.0 g/mol. • 34.0 g/mol/ 17.0 g/mol = 2 • The empirical formula HO becomes the molecular formula H2O2 !

  30. Finding Molecular Formulas :-) • Find the molecular formula of a cmpd with a molar mass of 60.0 g/mol and an empirical formula of CH4N. • C2H8N2 • Find the m.f. of a cmpd with a m.m of 62.0 g/mol and an e.f. of CH3O. • C2H6O2

More Related