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Stoichiometric Calculations Foldable. Obtain 3 sheets of paper. Stagger the pages about ¾ of an inch. Fold over so you have multiple flaps.

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Presentation on theme: "Stoichiometric Calculations Foldable. Obtain 3 sheets of paper. Stagger the pages about ¾ of an inch. Fold over so you have multiple flaps."— Presentation transcript:

1 Stoichiometric Calculations Foldable

2 Obtain 3 sheets of paper. Stagger the pages about ¾ of an inch. Fold over so you have multiple flaps.

3 Titles of Pages Stoichiometric Calculations Mole to Mole Mole to Mass / Mass to Mole Mass to Mass Limiting Reactant Percent Yield

4 Page 1 - Top Open your book, on the top flap, write the following: Steps in all stoichiometric calculations: – Write a balanced equation – Identify the known and unknown, what do you have and what are you trying to find? – Set up the problem with the given information – Identify the mole ratio – Check your answer, does it make sense?

5 Page 1 – Bottom – Mole to Mole Mole of A to Mole of B Ex. How many moles of H 2 O are produced from 5.0 moles of H 2 ? – Balanced Eq: 2H 2 + O 2  2H 2 O – Known: 5.0 mol H 2, Unknown: mols of H 2 O = 5.00 mol H 2 O 5.0 mol H 2 2 mol H 2 2 mol H 2 O Mole Ratio

6 How many grams of NaCl are produced from 5 moles of Na? Balanced Eq: 2 Na + Cl 2  2 NaCl Known: 5 moles of Na Unknown: grams of NaCl Page 2- Bottom – Mass to Mole Mole of A to Mass of BMass of A to Mole of B How many moles of NaCl are produced from 35 g of Cl 2 ? Balanced Eq: 2 Na + Cl 2  2 NaCl Known: 35 g Cl 2 Unknown: moles NaCl 5 mol Na 2 mol Na 2 mol NaCl 1 mol NaCl g NaCl Mole Ratio = g NaCl 35 g Cl g Cl 2 1 mole Cl 2 2 mol NaCl = 0.99 mol NaCl

7 Page 3 – Bottom- Mass to Mass Mass of A to Mass of B Ex. How many grams of NO 2 are produced from 250 g of N 2 gas? Balanced Eq: N 2 + 2O 2  2NO 2 Known: 250 g of N 2 Unknown: grams of NO 2 = g NO 2 1 mol N g N 2 2 mol NO g NO g N 2 1 mol N 2 1 mol NO 2 Molar MassMole Ratio

8 Page 4 – Bottom – Limiting Reactants Same as all the other problems, you just have to do two of them. Do the problem with N 2 first. Balanced Eq: N 2 + 2O 2  2NO 2 Known: 25 g N 2, Unknown: g NO 2 = g NO 2 Now do the same problem with O 2 Same balanced equation Known: 35 g O 2,Unknown: g of NO 2 = g NO 2 If you have 25 g of N 2 and 35 g of O 2, how many grams of NO 2 is produced, which one is the limiting reactant? The excess reactant? 25 g N g N 2 1 mol N 2 2 mol NO 2 1 mol NO g NO 2 35 g O g O 2 1 mol O 2 2 mol O 2 2 mol NO 2 1 mol NO NO 2 O 2 is the limiting reactant, this reactant will determine how much product is made. NO 2 is the excess reactant, it will be left over after the reaction g NO 2 is produced

9 Page 5 – Bottom - % Yield Ex. Problem: When this experiment was performed in the lab, the chemist was able to produce g of NO g NO 2 = actual yield %Yield = actual yield Done the same way if you need to figure out the amount of product use the limiting reactant steps. We will use the same balanced equation: N 2 + 2O 2  2NO 2 We know that g NO 2 is produced. The amount of product you calculate from the limiting reactant problem is the theoretical yield g NO 2 = theoretical yield theoretical yield X 100 % Yield = X 100 = 96.3 %


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