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The Mole

The Mole. Chapter 10. Formula Mass:. Is what a single molecule “weighs” in amu’s (atomic mass units) Revision:. So, 1 molecule of Water (H 2 O) weighs: 2 x 1.01 (for H) + 1 x 16.00 (for O) = 18.02 amu’s. Example #2: What is the mass of 1 molecule of Sugar(Sucrose)? (C 6 H 12 O 6 )

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The Mole

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  1. The Mole Chapter 10

  2. Formula Mass: Is what a single molecule “weighs” in amu’s (atomic mass units) Revision: So, 1 molecule of Water (H2O) weighs: 2 x 1.01 (for H) + 1 x 16.00 (for O) = 18.02 amu’s

  3. Example #2: What is the mass of 1 molecule of Sugar(Sucrose)? (C6H12O6) C: 6 x 12.01 = H: 12 x 1.01 = O: 6 x 16.00 = Do other examples? a) CO2 b) (NH4)2CO3

  4. The Mole: First, let’s look at names that reflect numbers: 1 dozen = 1 baker’s dozen = 1 score = 1 gross =

  5. Let’s now focus on a particular isotope – Carbon-12 1 Carbon-12 atom weighs ______________ But this is an impractical measurement. We want to work in the mass unit of grams. So, how many atoms of Carbon-12 would it take to weigh 12.00 g.?

  6. Amadeo Avogadro (Italian, 1776-1856) calculated the number to be 6.022 x 1023 and is also known as a So now, the average atomic mass number also represents how many grams that element would weigh if you had 1 mole of that substance.

  7. So, 1 mole of Water weighs: H: 2 x 1.01 g/mole = 2.02 g/mole O: 1 x 16.00 g/mole = 16.00 g/mole  This # is known as the _____________(mass of 1 mole) of Water. Examples. Calculate the Molar Mass of the following: a.) SO2 b.) (NH4)3PO4

  8. Mole to Mass & Mass to Mole Conversions If we are given the # moles of a substance and we want to calculate how much it weighs (i.e. what’s its mass?), then we convert by using the _________________________! E.g. What is the mass of 1.50 moles of Water? 1.50 mol. Of H2O x 18.02g of H2O = 27.03g of H2O 1 1 mol. of H2O E.g.#2 What is the mass of 0.75 mol. Of Salt?

  9. Now, going the other way. How many moles are in 100.g of CO2 ? 100.g of CO2 x 1 mol. of CO2 = _______________ 1 44.01g of CO2 E.g.#2 How many moles are in a pound of Sugar?

  10. Converting from moles to molecules & vicy versi In these conversions, instead of using the _________________________, you use Avacado’sAvagadro’s Number. (NA) Ex. How many molecules are in 1.50 moles of Water? (remember: 1 mole = 6.02 x 1023 ) 1.50 mol. x 6.02 x 1023 molecules = ___________________ 1 1 mol. Ex.2) How many moles in 2.107 x 1024 molecules of Salt? 2.107 x 1024 molecules x ____= 3.50 moles 1 6.02 x 1023 molecules

  11. Do these in-class egg samples: 1.) How many molecules are in 0.02 moles of Sugar? 2.) How many moles are in 3.01 x 1023 molecules of O2? Let’s look at lots of molecules of Water.

  12. Time to draw a MOLE diagram I know what you’re thinking! Now we can do Mass to Molecules conversions & vicyversi. (Hint: it’s a 2 step Chain Method) Ex. How many molecules are in 12.0g (~½oz) of Water? 12.0g of H2O x_____________x________________________ 1 1 mol of H2O = 4.00 x 1023 molecules of H2O Ex. What does 9.03 x 1022 molecules of Vitamin C weigh? (Vitamin C = C6H8O6)

  13. Standard Molar Volume The Volume occupied by 1 mole of a gas is the Molar Volume. The Volume occupied by 1 mole of a gas @ STP is known as the Standard Molar Volume of a gas and is equal to 22.4 L.  @ STP V = 22.4 L/mol.  V = n x 22.4 L/mol. n So 1 mole of any gas occupies 22.4L @ STP, but their masses may be different.

  14. So 2 moles of a gas will occupy twice the space (Volume) of 1 mole. e.g. 2H2 + O22H2O (more examples: N2 + H2 NH3 ,…) And remember:1 mole = 6.02 x 1023 molecules

  15. (Diagram – New Mole Diagram)

  16. Add that to the mole diagram…

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