Unit 5  Part 7    Moles  Grams And  Liters
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Unit 5 Part 7 Moles Grams And Liters

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    Unit 5  Part 7    Moles  Grams And  Liters Unit 5 Part 7 Moles Grams And Liters Presentation Transcript

    • Part 7 – Moles into Grams and Liters
    • WEIGHING (MASSING) IN CHEMISTRY
      • Chemists use mass, and normally small masses such as grams.
      • However they must relate the mass of chemical back to the counting of individual atoms.
    • The Gram Atomic Mass (GAM)
      • gram atomic mass- the mass of one mole of an element.
      • The gram atomic mass numerically equals the atomic mass of the element in grams.
    • Example:
      • Find the gram atomic mass of the following elements:
        • Na, Hg, Fe, S
    • Gram Formula Mass (GFM)
      • gram formula mass- the mass of one mole of a compound.
      • For gram formula mass we add together the gram atomic masses of the elements which make up the compound.
    • Example
      • Find the gram formula mass of the following compounds:
        • CoCl 2 , H 2 O, H 2 S0 4
      • Name these compounds.
    • Converting between moles and grams of a substance.
      • Conversions between moles and the mass of a substance uses the gram atomic mass or gram formula mass.
    • To convert from moles to grams
      • 1. Find the gram formula mass of the compound or element your looking for.
      • 2. Determine the number of moles you were given.
      • 3. Multiply the number of moles by the gram formula mass.
    • Example
      • Find the mass of 0.160 mol H 2 O 2 .
      • Find the mass of 6.0 X 10 26 atoms of Be.
    • To convert from grams to moles
      • 1. Find the gram formula mass of the compound you are looking for.
      • 2. Determine the number of grams you were given.
      • 3. Divide the number of grams you were given by the gram formula mass.
    • Example
      • Find the number of moles in each of the following:
        • 333g SnF 2 .
        • 5.0 X 10 24 molecules of SnF 2 .
    • Try these on you own...
      • Find the mass in each of the quantities below
        • 10.0 mol Cr
        • 3.32 mol K
        • 2.4 mol N 2
      • Find the number of moles in each of the quantities below
        • 10g H 2 O 2
        • 15g Ca(NO 3 ) 2
        • 50g C 20 H 42
    • FINDING VOLUME IN CHEMISTRY
    • The Volume of a mole of gas
      • Although the volumes of 1 mol of a liquid or solid can vary greatly between different substances, the volume of 1 mol of the gas of any substance has the same volume, at equal temperature and pressure.
      • 1 mole of a gas of any substance occupies a volume of 22.4L at STP (standard temperature and pressure).
    • Standard Temperature and Pressure (STP)
      • Temperature and pressure can affect the volume of a gas.
      • In order to “standardize” experiments between scientist, we use a standard set of values to work with gases.
      • Standard Temperature = 0°C
      • Standard Pressure = 1 atm (air pressure at sea level)
    • Examples
      • Determine the volume, in liters, of 0.600 mol of SO 2 gas at STP.
    • Your turn…
      • What is the volume at STP of 0.960 mol CH4?
      • Assuming STP, how many moles are in 89.6 L SO 2 ?
    • Converting between units with moles
      • The mole is the most useful way for chemists to express the amount of matter.
    • Try these...
      • Determine the volume in liters of 50g of SO 2 gas at STP.