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
Free Pressure Ideal gas law Gas
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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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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Fuels Investigation Aim: To find out which fuel gives out the most energy. Planning We will be using 6 different fuels to heat up 100ml of water‚ and find out the changes of the temperature. We will measure the temperatures of the water before and after the experiment. We will burn heat the water for exactly 2 minutes‚ and check the changes in temperature. The change in temperature will allow us to work out the energy given off the fuel by using this formula: Mass of water x 4.2 (water’s specific
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needed to form the I3- complex. In this type of analysis‚ excess iodide is added to the oxidizing agent‚ and the triiodine is titrated with stand thiosulfate. This indirect analysis finds the number of moles of ascorbic acid based on the known number of moles of IO3- and subtracting half the amount of moles of the thiosulfate solution. II: Equations: Iodate with Iodide: IO3- + 8I- + 6H+ 3I3- + 3H2O Thiosulfate with Triiodide 2S2O32- + I3- S4O62- + 3I- Ascorbic Acid with Triiodide
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Mg2+ (aq) + 2Cl- (aq). The major findings of this experiment were that there was a chemical reaction between hydrochloric acid and magnesium‚ and the reaction produced the hydrogen gas. The results also indicated how many moles of hydrogen gas were equal to the amount of moles of magnesium consumed. Procedure Step 1:
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concentration = moles / volume 0.10=moles/0.010 Moles of Cu (NO3)2 (aq) = 0.001 moles Mass of empty bottle = 6.00grams Mass of empty bottle +copper metal =6.05grams Mass of copper metal recovered after the experiment = 0.050 grams Finding moles of copper: Moles = mass/ Mr = 0.050 / 63.55 =0.00079 moles
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Processing Raw Data : Part 1 Equation of the reaction; Mg(s) + 2HCl(ℓ) → MgCl2(aq) + H2(g) no of moles : no of moles of Mg = mass/molar mass = 0.31g___ 24.31g/mol = 0.01275 moles no of moles of HCl = molarity x volume = 1.0M x (25/1000)mL = 0.025 moles heat of reaction will be 0.025 moles as HCL act as the limiting reactant. Enthalpy change of the reaction‚H2 Volume of HCL solution =
Free Thermodynamics Enthalpy Measurement