Experiment #5 Avagadro’s Number 6.02 x 10 23 And The Standard Deviation x  S.

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Experiment #5 Avagadro’s Number 6.02 x And The Standard Deviation x  S

Introduction ► ► Purpose:   Relate a gram formula weight to Avogadro’s number by using the dimensional analysis approach and determine the correct number of significant figures in your applications.   Compute the standard deviation for the volume of water delivered by a 10 mL Graduate Cylinder.

Key Ideas ► ► Amu Vs. Gram – ► ► Atom Vs. Ion – ► ► Atom Vs. Mole – ► ► Formula Weight – ► ► GFW,GAW,GMW – ► ► Dimensional Analysis – ► ► Standard Deviation –

Just How Big is a Mole? ► Enough soft drink cans to cover the surface of the earth to a depth of over 200 miles. ► If we were able to count atoms at the rate of 10 million per second, it would take about 2 billion years to count the atoms in one mole.

Volume of a penny x mm 3

Volume of Earth = ~ ×10 18 mm³

Volume of Jupiter = ×10 21 mm³ Jupiter

Atom Vs. Mole Mole 6.02X10 23 Atoms Larger mass measured in grams Larger in size Can be seen Atom 1 Atom Very small mass measured in Amus Very Small in size Can’t be seen

Amu Vs. Gram Amu – We use if we are talking about the mass of an atom. Ex. the mass of an iron atom is 55.8 amus. Gram – We use if we are talking about the mass of a mole or fraction of a mole. Ex. The mass of one mole of iron is 55.8 grams.

Formula weight – the mass of the collection of atoms represented by a chemical formula. For Ex. water contains two hydrogen atoms and one oxygen atom. 1 x (mass of O) = x 1.01 (mass of H) = Formula Weight  The formula weight tells us the mass of one mole of our substance. Formula Weight

GFW – Gram Formula Weight This refers to the mass of an ion or ionic compound Ex. Mass of a Cl - GAW – Gram Atomic Weight This refers to the mass of a atom Ex. Mass of a Cl atom GMW Gram Molecular Weight This refers to the mass of a molecule or molecular compound Ex. Mass of one molecule of H 2 O

How do Avagadro’s number, Mole and GAW Apply to each other? ► ► One mole of Tin has a mass of g. ► ► One atom of Tin has a mass of Amu. ► ► One mole of Tin contains 6.02X10 23 atoms.

Dimensional Analysis Convert 10 m to mm Remember 1 m = 1000mm They both mean the same thing it all depends on what you need.

Dimensional Analysis # 1 # 3 # 2 Mult. left to right divide top to bottom What you are given always over 1 The 1 is a filler. The unit you want to eliminate is placed in the lower right so it will cancel out with your original unit.

Keep in mind X going and / going

Ex#1 pg 51 Find the # of moles in the sample of Tin. Given the sample has a mass of 29.04g

Chart on pg 55 “Everything is based off of one mole ” To determine the g formula wt. determine the atomic mass of all atoms present Example 1 mole of H 2 O – 18.00grams

Chart on pg 55 “Everything is based off of one mole ” To determine #g / molecule Find the # grams per mole / number of molecules Example 2 1 mole of H 2 O = 18.00grams 18.00grams / 6.02x10 23 molecules = 2.9x #g/molecule = 2.9x10- 23

Chart on pg 55 “Everything is based off of one mole ” To determine # of moles use dimensional analysis Grams to moles Example g Cu 1 mol Cu 63.5 g Cu =.58mol

Chart on pg 55 “Everything is based off of one mole ” To determine the number of atoms per mole add up the number of atoms in the formula Example 4 H 2 O = 3 atoms

Standard Deviation ► ► This is how much your value is off from the actual answer. Can be used as a correction factor. ► ► Ex. A 1mL pipette delivers 1mL + or -.007mL   So the pipette delivers.9993mL or mL. X = Avg

Standard Deviation Ex. 1 mL Pipette 1.02gM H 2 O1.01g 1.02g Density of H 2 0 = g/mL 1.02mL 1.01mL1.02mL1.01mLVol. of pipet Use V= M/D to determine volume delivered Mass of Beaker & water g111.53g109.50g g g Mass of Beaker g

N= number of trials ∑ (Xi-X avg.) 2 Xi-Xavg. (a) =.01 (b) = 0 (c) =.01 (d) = 0 (e) = 0 X avg.= 1.02 mL #1 #2 #3 ( Xi-Xavg. ) 2 (a).01 =1.0X10 -4 (b) 0 = 0 (c).01 =1.0X10-4 (d) 0 = 0 (e) 0 = 0 #4 #5∑(Xi-X avg.) 2 /N-1 #6 Take Square Root of Step #5 Final Answer: +/ mL.

Due Next Week ► ► Pages 51 & 53 we are determining the number of atoms / ions or moles that are asked for. ► ► YOU MUST SHOW ALL WORK FOR CREDIT!! ► ► Page 55 complete the table and show all work. ► ► Pages 61 determine the St. Dev. for 1 mL pipette ( I do as a example) ► ► Page 63 determine the St. Dev. for a 10mL. graduated cylinder.