(II) Sulfate Purpose: The purpose of this lab is to find out how many moles of water there are in one mole of Copper Sulfate (CuSO x HO) and the percent by mass of water in the hydrate. This will be accomplished by heating a determined mass of the hydrate to remove the water‚ and by measuring the salt left over. Introduction: This laboratory experiment will be done to find out how many moles of HO are present per one mole in the hydrate CuSO. A hydrate is a compound that has a fixed number of
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- Mass of crucible and anhydrous salt (31.39g) = .96g 3. How many moles of water is this?
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you can buy bananas by the pound. The third and last way to quantify or measure matter is to determine its volume. For example‚ people by gasoline by the gallon. Chemists use a unit that is a certain number of particles. This unit is known as the mole. A mole is the quantity of anything that has the same number of particles found in 12.000 grams of carbon-12. That number of particles is Avogadro’s Number which is about 6.02 x 1023 ‚ representative particles. That is an SI unit for measuring the
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Chapter 6 – Properties of gases lecture notes 1. Gas phase Gases have neither definite shape or volume 1) volume changes with pressure 2) volume changes with temperature 3) gases are miscible 4) gases are generally MUCH less dense than liquids 2. Atmospheric pressure 1 atm = 760 torr (mm of Hg) F= ma F = force m = mass a = acceleration P = F/A - ma/A P = pressure
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find: i. Mass ii. Mole iii. Divide each mole by lowest mole value iv. Whole number ratio of each element 2. Examples: v. 75% C‚ 25% H Basis: 100g a. Mass: C = 75g‚ H = 25g b. Recall from Table T: mole = massatomic mass Mole C = 75g12g/mole = 6.25 moles Mole H = 251 g/mole = 25 moles c. Mole C = 6.25 moles6.25 moles = 1 Mole H = 25 moles6.25 moles = 4 d. CH4 vi. 13% Mg‚ 87%
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What is molar mass?Molar mass is the weight of one mole (or 6.02 x 1023 molecules) of any chemical compounds. Molar masses of common chemical compounds that you might find in the chemistry laboratory can range between 18 grams/mole for compounds like water to hundreds of grams per mole for more complex chemical compounds.The lightest possible chemical that one can have under normal conditions is hydrogen gas‚ or H2. There is no limit to how heavy a chemical compound can be - it is not uncommon for macromolecules (large
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Mise-en-scène. The arrangement of everything that appears in the framing – lighting and costume – is called mise-en-scène Rocky’s mise-en-scene :audience understand more about the character Adrian. and how she changes in her personality when she meets Rocky. At the time Rock walks into the pet shop where Adrian works‚ the filmmaker lets people see her as an old-fashioned girl. She wears a grey cardigan‚ old-fashioned shirt and cat-eye glasses like a homemaker. She also is a unconfident and quiet girl;
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0.6‚ 0.7‚ 0.8 and 0.9 to form several complexes. Using the UV-Vis Spectrometer‚ the absorbances are taken at wavelengths 530‚ 545‚ 578‚ 622 and 640 nm due to the emergence of several complex compositions. The values of corrected absorbances and the mole fraction of en (X) are plotted to obtain a curve. From these curves‚ an intersection from the 2 trend lines are determined‚ denoting the values of x‚ needed for the determination of n. The process led the group with similar values of n which is 1‚
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Aim: To react NaHCO3 with HCl to form NaCl and two other products and then calculate the mole relationships between NaHCO3 and NaCl and calculate a balanced equation for this reaction. Safety: • Wear safety goggles at all time • Handle all chemicals with care • Use equipment like tongs when handling warm/hot objects • If chemicals are spilt on self‚ wash off immediately • Stand at all times Hypothesis: The NaHCO3 will react successfully with the HCl and will form NaCl‚ H2O and
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Research Methods for Business Students has guided hundreds of thousands of student researchers to success in their research proposals‚ projects and dissertations. Research methods for business students fifth edition Mark Saunders Philip Lewis Adrian Thornhill ● Start your research with confidence and complete it with success. Cover photograph: Eastcott Momatiuk/ Getty www.pearson-books.com CVR_SAUND6860_05_SE_CVR.indd 1 26/2/09 18:08:14 A01_SAUN6860_05_SE_FM.QXD 12/2/09
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