Do Now. Agenda Welcome back! The beginning of ALL THE MATH! Homework PBJ procedure Pages 1-3 of HW packet

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1 Do Now Agenda Welcome back! The beginning of ALL THE MATH! Homework PBJ procedure Pages 1-3 of HW packet

2 All the math

3 Molar Mass the mass of one mole of any substance, reported in grams (gram atomic mass)

4 Molar mass sum of the molar masses of the elements in the compound Example: CH 4 Element # mol element/mol compound Molar Mass Mass contribution C g/mol g H g/mol 4.04 g The molar mass of CH 4 =16.05 g/mole

5 For example, the molar mass for the element, Al, is g. This means that 1 mole of Al atoms has a mass of 27.01g. In other words, 6.02 x Al atoms has a mass of g.

6 Relative amounts of each element in a compound Can be used as a conversion factor

7 What is the percent by mass of nitrogen in NH 3? MM of NH 3 : g/mol Mass contribution of N: g/mol (14.01g/mol) (17.04g/mol) * 100 = 82.22%

8 We use it to count, just like we use dozen or pair. If we have: 1 dozen roses= 12 roses If we have one mole of anything: We have 6.02x10 23 of that thing Avogadro s number

9 A chemical formula showing the lowest whole # ratio of elements in a compound Can be calculated from percent composition Example: Find the empirical formula for a compound that is composed of 62.1% C, 13.8% H, and 24.1% N.

10 To determine formula: Convert the masses of each element into moles. Divide each mole value by the smallest mole value to get mole ratio Write empirical formula using symbols, and use the whole-number ratio as subscript. Non-whole numbers multiply by 2 or 3 to make them whole

11 C 62.1g H 13.8g N 24.1 g

12 will be identical to or some multiple of the empirical formula. Show the actual number of each kind of atom present Example: C 2 H 6 =Molecular Formula CH 3 =Empirical Formula Example: CH 4 =Molecular Formulas CH 4 =Empirical Formula

13 Steps *Find empirical formula *Calculate molar mass for empirical formula *Divide MM molecular/mm empirical *Multiply this factor by each of subscripts in empirical formula to give molecular formula

14 Three steps: List the knowns and the unknown. Solve for the unknown. Select the appropriate unit equality and make it into a conversion factor, with the unknown s unit in the numerator and the known s unit in the denominator. Multiply the known quantity by the conversion factor. Make sure to eliminate all but the unknown s unit. Evaluate - Does the result make sense? Chapter 10

15 We use moles to count particles like: atoms, molecules, formula units, or ions. One mole of moles (the animal) would have the equivalent mass to 60x the Earth s oceans.

16 How many atoms are there in 1 mole of sodium? 6.02x10 23 atoms How many formula units are there in 1 mole of KOH? 6.02x10 23 formula units How many molecules are there in one mole of water? 6.02x10 23 molecules

17 Example: How many moles of water molecules are in 1.21 x water molecules?

18 Example: How many Cu atoms are in 2.54 moles of Cu atoms?

19 If you are given a certain mass of a substance, you can find out how many moles you have by using the molar mass. Example: How many moles of carbon atoms are found in g of carbon? 24.02g x (1mole) = moles C (12.01g)

20 One mole of any gas at STP occupies a volume of 22.4L. S.T.P.-Standard Temperature and Pressure. The values are 0 Celsius and 1 atmosphere of pressure. Example: What is the volume of 2.55 moles of hydrogen

21 Mass molar mass 1.00 mol 1.00 mol molar mass MOLE 6.02x10 23 particles 1.00 mol 1.00 mol 6.02x10 23 particles Particles 22.4 L 1 mol 1 mol 22.4 L Volume (gas at STP)

22 The calculation of quantities in chemical reactions A balanced chemical equation becomes a recipe that we can use

23 2Na + Cl 2 2NaCl In the above equation, the coefficients tell you: The relative number of particles The relative number of moles If and only if all substances are gaseous, the relative number of

24 How many moles of chlorine gas are needed to react with excess sodium to produce 5.00 moles of sodium chloride?

25 A unit of concentration Units are mole solute/liter solution Conversion factor!

26 If you dissolve 5 moles of NaCl in enough water to produce 1 L of solution, what is the concentration?

27 How many grams of water can be produced when grams of oxygen react with excess hydrogen?

28 2H 2 (g) + O 2(g) 2H 2 O (g) Example: How many liters of S.T.P. are needed to completely react with 6.0 liters of hydrogen to produce water?

29 Measurement of efficiency of a reaction

30 A factory worker in a paint company follows a batch slip to prepare a 1500 gallon batch of paint. However, when the batch goes to the filling department only 1489 gallons are filled. What is the % yield?

31 As in the cookie recipe, if you run out of eggs (and can t get more), but have the rest of the recipe, you can t make any more cookies. In chemistry we call the reactant that runs out first, the limiting reactant/reagent. All other reactants that we have in excess we call excess reagents.

32 2H 2 + O 2 2H 2 O If 40.00g of hydrogen react with g of oxygen, what mass of water will be produced?

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