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Entry Task: March 11 th Monday

Entry Task: March 11 th Monday. Entry task question: 2AgCl + Mg  MgCl 2 + 2Ag Question: How many grams of silver can be produced if 500.0 grams of magnesium reacts with excess AgCl ? You have ~10 minutes. Agenda:. Sign off and Discuss Stoichiometry #3 ws

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Entry Task: March 11 th Monday

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  1. Entry Task: March 11th Monday Entry task question: 2AgCl + Mg  MgCl2 + 2Ag Question: How many grams of silver can be produced if 500.0 grams of magnesium reacts with excess AgCl? You have ~10 minutes

  2. Agenda: • Sign off and Discuss Stoichiometry #3 ws • Notes on Limited Reactants

  3. Copper II sulfate reacts with potassium phosphate to create copper II phosphate and potassium sulfate ___CuSO4 + ___K3PO4 ___K2SO4 + ___Cu3(PO4)2 3 2 3

  4. ___CuSO4 + ___K3PO4 ___K2SO4 + ___Cu3(PO4)2 3 2 3 How many grams of copper II sulfate is needed to produce 45.0g of potassium sulfate? 45.0 grams K2SO4 1 mole of K2SO4 3 mole of CuSO4 159.54 g of CuSO4 g of CuSO4 3mole of K2SO4 174.257 g of K2SO4 1 mole of CuSO4 21537.9 41.2 g of CuSO4 522.77

  5. ___CuSO4 + ___K3PO4 ___K2SO4 + ___Cu3(PO4)2 3 2 3 If 74.9 grams of potassium sulfate is produced from this reaction , how much copper II phosphate can be produced? 74.9 grams K2SO4 1 mole of K2SO4 1 mole of Cu3(PO4)2 380.578g of Cu3(PO4)2 g of Cu3(PO4)2 3mole of K2SO4 174.287 g of K2SO4 1 mole of Cu3(PO4)2 28505.29 54.5 of Cu3(PO4)2 522.861

  6. ___CuSO4 + ___K3PO4 ___K2SO4 + ___Cu3(PO4)2 3 2 3 How many grams of potassium phosphate are needed to react with 75.0 grams of copper II sulfate to complete the reaction? 75.0 grams CuSO4 1 mole of CuSO4 2 mole of K3PO4 211.97g of K3PO4 g of K3PO4 3mole of CuSO4 159.54 g of CuSO4 1 mole of K3PO4 31795.5 66.5 g of K3PO4 478.62

  7. ___CuSO4 + ___K3PO4 ___K2SO4 + ___Cu3(PO4)2 3 2 3 If there are 2.09 grams of potassium phosphate produced in this reaction, how much copper II sulfate is required? 2.09 grams K3PO4 1 mole of K3PO4 3 mole of CuSO4 159.54g of CuSO4 g of CuSO4 2 mole of K3PO4 211.97 g of K3PO4 1 mole of CuSO4 1000.32 2.36 g of CuSO4 423.94

  8. ___CuSO4 + ___K3PO4 ___K2SO4 + ___Cu3(PO4)2 3 2 3 How many grams of potassium phosphate will be needed to produce 64.5 grams of copper II phosphate? 64.5 grams Cu3(PO4)2 1 mole of Cu3(PO4)2 2 mole of K3PO4 211.97g of K3PO4 g of K3PO4 1 mole of Cu3(PO4)2 380.58 g of Cu3(PO4)2 1 mole of K3PO4 27344.13 71.8 g of K3PO4 380.58

  9. ___CuSO4 + ___K3PO4 ___K2SO4 + ___Cu3(PO4)2 3 2 3 If there are 1.25 grams of copper II phosphate produced in a reaction, how much potassium phosphate is required? 1.25 grams Cu3(PO4)2 1 mole of Cu3(PO4)2 2 mole of K3PO4 211.97g of K3PO4 g of K3PO4 1 mole of Cu3(PO4)2 380.58 g of Cu3(PO4)2 1 mole of K3PO4 529.25 1.39 g of K3PO4 380.58

  10. I can • Identify the limiting reactant in a chemical equation • Identify the excess reactant and calculate the amount remaining after the reaction is complete. • Calculate the mass of a product when the amounts of more that one reactant are given

  11. Limiting Reactant • There are 2 types of reactants in a chemical reaction • After a reaction, the reactant is said to be in excess (there is too much). • The other reactant limits how much product we get. Once this reactant runs out, the reaction s. This is called the limiting reactant.

  12. Limiting Reactant • To find out which reactant in the chemical reaction is the limiting reactant, we have to try each reactant involved in the reaction. • We have to calculate how much of product we can get from each reactant to determine which is the limiting one. • The lower amount of product is the correct reactant (limited reactant). • When you pick a product for your calculations, use the same product in your comparison.

  13. 10.0g of aluminum reacts with 35.0 grams of chlorine gas to produce aluminum chloride. Which reactant is limiting, which is in excess, and how much product is produced? 2 Al + 3 Cl2 2 AlCl3 10.0 g Al 1 mole Al 133.5 g AlCl3 2 mol AlCl3 49.4 g AlCl3 27.0 g Al 2 mole Al 1 mol AlCl3 35.0g Cl2 1 mole Cl2 2 mole AlCl3 133.5 g AlCl3 43.5 g AlCl3 3 mole Cl2 71.0 g Cl2 1 mole AlCl3

  14. Which reactant is Limited and which reactant is Excess? 2 Al + 3 Cl2 2 AlCl3 Excess = Al 10.0 g Al 1 mole Al 133.5 g AlCl3 2 mol AlCl3 49.4 g AlCl3 27.0 g Al 2 mole Al 1 mol AlCl3 Limited= Cl2 35.0g Cl2 1 mole Cl2 2 mole AlCl3 133.5 g AlCl3 43.5 g AlCl3 3 mole Cl2 71.0 g Cl2 1 mole AlCl3

  15. 10.0g of aluminum reacts with 35.0 grams of chlorine gas to produce aluminum chloride. Which reactant is limiting, which is in excess, and how much product is produced? 2 Al + 3 Cl2 2 AlCl3 Start with the limited reactant!! Used In reaction 35.0g Cl2 1 mole Cl2 2 mole Al 26.98 g Al 8.9 g Al 3 mole Cl2 71.0 g Cl2 1 mole Al Given Used In reaction 1.1 g EXCESS 10.0 grams Alminus 8.9 g Al =

  16. 15.0 g of potassium reacts with 15.0 g of iodine. Calculate which reactant is limiting and how much product is made AND how much excess. 2 K + I2 2 KI 15.0 g K 1 mole K 165.99 g KI 2 mol KI 63.68 g KI 39.098 g K 2 mole K 1 mol KI 15.0 g I2 1 mol I2 2 mol KI 165.99 g KI 19.6 g KI 1 mol I2 253.8 g I2 1 mol KI

  17. Which reactant is Limited and which reactant is Excess? 2 K + I2 2 KI Excess = K 15.0 g K 1 mole K 165.99 g KI 2 mol KI 63.68 g KI 39.098 g K 2 mole K 1 mol KI Limited= l2 15.0 g I2 1 mol I2 2 mol KI 165.99 g KI 19.6 g KI 1 mol I2 253.8 g I2 1 mol KI

  18. 15.0 g of potassium reacts with 15.0 g of iodine. Calculate which reactant is limiting and how much product is made AND how much excess. 2 K + I2 2 KI Start with the limited reactant!! Used In reaction 15.0 g I2 1 mol I2 2 mol K 39.1 g K 4.62 g K 1 mol I2 1 mol K 253.8 g I2 Given Used In reaction 10.38 g EXCESS 15.0 grams Kminus 4.62 g K =

  19. Limiting Reactant: Recap • You can recognize a limiting reactant problem because there is MORE THAN ONE GIVEN AMOUNT. • Convert ALL of the reactants to the SAME product (pick any product you choose.) • The lowest amount of product involved the reactant which is the LIMITING REACTANT. • The other reactant(s) are in EXCESS. • Start with limited reactant and compare it with the other reactants in a gram to gram Stoichiometry conversation. • Then find the amount of excess, subtract the amount used from the given amount.

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