Name _________________________________________ Date ______________ Period ______________ Chemistry Lab Mole: Measuring Mass as a Means of Counting Purpose: Determine the number of atoms that fit on one tea spoon. 1. Use one clean and dry 50 mL beaker. Place on a balance and press the zero button until the display shows 0.00. 2. Place one level teaspoon of sodium chloride (NaCl) into the beaker‚ determine the mass and record in the table (row 1). 3. Repeat steps 1-2 for CaCO3 4. Repeat steps 1-2
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Moll Flanders‚ A Fallen Angel Moll Flanders‚ the main character in the book The Fortunes & Misfortunes of the Famous Moll Flanders‚ written by Dafoe‚ is telling her life story in this book. The reader can see how her life rise and fall‚ how she is a maid‚ then become a wife in a rich family‚ up and down‚ and then fall into the criminal world. She is a dynamic character. Her up and down life‚ mostly down‚ causes her character to change throughout the novel. Dafoe has succeed to create a Moll that
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of substance mole mol Electric Current ampere A Luminous Intensity candela cd Prefixes for Units giga- G 109 mega- M 106 kilo- k 103 deci- d 10-1 centi- c 10-2 milli- m 10-3 micro- u 10-6 nano- n 10-9 pico- p 10-12 femto- f 10-15 atto- a 10-18 B. The mole and millimole 1. Mole – amount of a chemical species. Avogadro’s number 6.022 X 1023 of particles. 2. Millimole – 1mmol = 10-3 mol 3. Molar mass – mass in grams of one mole of a substance
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1 mole of any substance can be defined as: Amount of a substance that contains as many particles (atoms‚ molecules or ions) as there are atoms in 12 g of the 12C isotope Avogadro number or Avogadro constant (NA); equal to 6.022 × 1023 particles Example − 1 mole of oxygen atoms = 6.022 × 1023 atoms 1 mole of carbon dioxide molecules = 6.022 × 1023 molecules 1 mole of sodium chloride = 6.022 × 1023 formula units of sodium chloride Molar mass of a substance can be defined as: Mass of one mole
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Shawn Dubbs Lab 1 The Mole Concept of and the Chemical Formula of a Hydrate Abstract: The objective of this lab was to conduct an experiment to analyze the molar components in alum. This was conducted by heating the alum till the water had evaporated and then determining the number of moles for each component. Then using the these amounts to figure out the empirical formula for alum. Results: In order to determine how much of each separate component a total mass was taken before hand for
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of each element in BaCo3‚ assume we have 1 mole of BaCo3‚ we have M(Baco3)g=137.3+12.0+3x16.0=197.3g/mol so we have 197.3g Baco3 so 1mol of Ba=…… 8. %element=m(element)/m(compound)x100% 9. Empirical formula-----simplest whole number ratio Metallic elements and ionic substances--- EF=formula Covalent substances---EF may be the same or simple whole number ratio of the empirical formula. 10. mass(g) m/M moles(mol) divide by smallest simplest mole ratio-----EF 11. If it doesn’t give the exact
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lab we took Fe(NO3)3 and NaOH and mixed 7 different mole ratios in graduated cylinders to determine what the mole ratio is. We also did the same thing with solutions of CuCl2 and Na3PO4. We determine the mole ratios by graphing the volume of reactant #1 vs. volume of precipitate for each reaction. Data Part 1.) Cylinder 1 2 3 4 5 6 7 Fe(NO3)3‚ 0.1 M‚ ml 5 10 12 15 17 20 24 NaOH‚ 0.1 M‚ ml 55 50 48 45 43 40 36 Fe:OH mole ratio 1:11 1:5 1:4 1:3 2:5 1:2 2:3 Volume Precipitate
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Name Mole Lab Exercises I. Pre Lab Questions Answer the following questions. (Hint: Your textbook will be helpful.) 1. ‘s number is the number of carbon atoms that are present in 12 g of 12C. 2. How many molecules of a compound are in one mole of that compound? 3. Write out the formula for finding percent by mass. 4. Write out the formula for finding Molarity. 5. The Formula Weight of a compound is equal to mole of that compound.
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S. 5.2 – The Mole The mole: - - - - Ex. - Molar mass (g/mol): - - - Ex. |Element |Atomic mass shown on Periodic |Molar mass of element | | |table | | |N |14.0067 |14.0067 g
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underlying purpose in determining the relationship between moles evolved and consumed. This can be demonstrated by measuring the hydrogen gas evolved by performing a chemical experiment when hydrochloric acid reacts with the magnesium. The formulated reaction includes; Mg + 2HCl → H2 + Mg2+(aq) + 2Cl- (aq) The major findings contributing to the experiment is being able to determine and distinguish what moles have evolved thus being the hydrogen moles evolved allowing the magnesium to be consumed within
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