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Define mole ratio (What is it? How is it determined?)

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Presentation on theme: "Define mole ratio (What is it? How is it determined?)"— Presentation transcript:

1 Define mole ratio (What is it? How is it determined?)
Q of the Day In your own words: Define mole ratio (What is it? How is it determined?) Day

2 Define mole ratio (What is it? How is it determined?)
Q of the Day In your own words: Define mole ratio (What is it? How is it determined?) Day PERIOD 3

3 Q of the Day At STP 44.8 liters of water vapor were produced via a composition (synthesis) reaction. How many moles of O2 were used? Day PERIOD 1

4 Practice Period 1 2Al(s) + 3CuCl2(aq)  2AlCl3(aq) + 3Cu(s) According to the reaction above if you start with about 27 grams of aluminum how much copper should you produce (in grams)? What is this calculation called?

5 4NH3(g) + 6NO(g) 5N2(g) + 6H2O(l)
Stoichiometry Reaction Stoichiometry – relates quantities of reactants and products in chemical reactions Mole ratio – conversion factor that relates the amounts in moles of any two substances involved in a chemical rxn Example: 4NH3(g) + 6NO(g) N2(g) + 6H2O(l)

6 Stoichiometry Mole ratio – just another player in the conversion game
- Used to change from one substance to another - Does NOT change units - Does change substance

7 Converting: Molar mass = Avogadro’s number = Avogadro’s law = =
Mass to moles Moles to mass Moles to atoms / molecules / particles Atoms / molecules / partilces to moles Moles to liters Liters to moles Changing a substance = Avogadro’s number = Avogadro’s law = = Mole ratio

8 Mole ratios are exact – do not limit sig. figs.
Stoichiometry Mole ratio – just another player in the conversion game Mole ratios are exact – do not limit sig. figs.

9 4NH3(g) + 6NO(g) 5N2(g) + 6H2O(l)
Stoichiometry 4NH3(g) + 6NO(g) N2(g) + 6H2O(l) __?__ Start with 20 mols NH mols N2 Start with 20 grams NH moles NO Start with 20 grams NO grams N2

10 4NH3(g) + 6NO(g) 5N2(g) + 6H2O(l)
Stoichiometry 4NH3(g) + 6NO(g) N2(g) + 6H2O(l) __?__ Start with 20 mols NH molecules N2 Start with 20 grams NH molecules NO 1.5e25 molecules N2 1.1e24 molecules NO Start pd 1

11 STEPS FOR SOLVING: Identify the Balanced chemical equation
Identify what you know and what you need to know Get an idea of what you need to do Start your conversion

12 Q of the Day At STP 44.8 liters of water vapor were produced via a composition (synthesis) reaction. How many moles of O2 were used? Day PERIOD 3

13 Stoichiometry If you produce 116 grams of sodium chloride by reacting sodium and chlorine how many mols of sodium must you have used? 2Na + Cl2 → 2NaCl 116 g NaCl = ____ mols Na answer = 2 mols Na

14 Stoichiometry Cupric chloride decomposes and 127 grams of solid copper form. How many liters of chlorine gas are produced at STP? CuCl2 → Cu + Cl2 127 g Cu = ____ liters Cl2 answer = 44.8 liters Cl2

15 Limiting Reactants Limiting Reactant – the reactant that limits the amounts of the other reactants that can combine and the amount of product that can form in a chemical reaction – the one you will run out of Excess Reactant – any substance that is not used up completely in a reaction – left over

16 Assignment

17 SOLVE: 1.5e24 molecules of SO2 = ____ grams of SO2? S2 + 2O2  2SO2
Q of the Day SOLVE: 1.5e24 molecules of SO2 = ____ grams of SO2? S2 + 2O2  2SO2 And how many moles of S2? Day

18 LAB


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