# Do Now: 9/8 AgNO 3(aq) + CaCl 2(aq) --> Ca(NO 3 ) 2(aq) + AgCl (s) 1.What is the molar mass of Silver Nitrate? (AgNO 3 ) 2.What does it mean to have a.

## Presentation on theme: "Do Now: 9/8 AgNO 3(aq) + CaCl 2(aq) --> Ca(NO 3 ) 2(aq) + AgCl (s) 1.What is the molar mass of Silver Nitrate? (AgNO 3 ) 2.What does it mean to have a."— Presentation transcript:

Do Now: 9/8 AgNO 3(aq) + CaCl 2(aq) --> Ca(NO 3 ) 2(aq) + AgCl (s) 1.What is the molar mass of Silver Nitrate? (AgNO 3 ) 2.What does it mean to have a balanced reaction? 3.Is this one balanced? If not balance it. 4.Why do we balance reactions? 5.If you use 15.0 g of AgNO 3, how many grams of Ca(NO 3 ) 2 will be produced assuming you have plenty of CaCl 2 ?

Unit 8 - Stoichiometry Reaction Stoichiometry

Where do we use stoichiometry?  To determine:  how much of the other reactants are needed  how much of each product should be produced  limiting reactants

Mole Ratio in reactions 2 H 2 + O 2  2 H 2 O Coefficients can represent moles in balanced reactions. 2 moles of hydrogen burn with 1 mole of oxygen to form 2 moles of water.

Mole Ratio 2 H 2 + O 2  2 H 2 O Possible mole ratios/ conversion factors: 2 H 2 -to-1 O 2 2 mol H 2 1 mol O 2 2 H 2 O-to-2H 2 2 mol H 2 O 2 mol H 2 2 H 2 O-to-1 O 2 2 mol H 2 O 1 mol O 23 others exist

1) Balance this equation: HgO  Hg + O 2 2) What is the mole ratio between HgO and O 2 ? 3) If you start with 10 moles of HgO, how many moles of O 2 would you make? 2 2 mol HgO 1 mol O 2 10 mol HgO X 1 mol O 2 = 5 mol O 2 2 mol HgO

 2HgO  2Hg + O 2 1) What is the mole ratio between HgO and Hg?  2) If you start with 10 moles of HgO, how many moles of Hg would you make? 2 mol HgO 2 mol Hg 10 mol HgO X 2 mol Hg = 10 mol Hg 2 mol HgO

2HgO  2Hg + O 2  If you start with 100 g of HgO how many moles of O 2 would be formed in the reaction? 100 g HgO X 1 mol HgO X 1 mol O 2 = 0.23 mol O 2 216.59 g HgO 2 mol HgO

 If you start with 20.7 g of HgO how many moles of Hg would be formed in the reaction?

What is the mass of HgO you need to form 10.0 grams of O 2 From this reaction? HgO  Hg + O 2 2 10.0 g O 2 X 1 mol O 2 X 2 mol HgO X 216.59 g HgO =135.4 g HgO 32 g O 2 1 mol O 2 1 mol HgO

All Class Practice:  H 2 SO 4 + 2NaOH  Na 2 SO 4 + 2H 2 O  How many moles of NaOH do you need to react with 1.00 mole of H 2 SO 4 ?  How many moles of NaOH do you need to react with 32.7 moles H 2 SO 4 ? 32.7 mol H 2 SO 4 X 2 mol NaOH = 65.4 mol NaOH 1 mol H 2 SO 4 1.00 mol H 2 SO 4 X 2 mol NaOH = 2.00 mol NaOH 1 mol H 2 SO 4

All Class Practice:  H 2 SO 4 + 2NaOH  Na 2 SO 4 + 2H 2 O  How many moles of H 2 SO 4 do you need to react with 20.0 g NaOH?  How many grams of Na 2 SO 4 will be produced if 27.6 g NaOH is reacted with excess H 2 SO 4 ? 2O.0 g NaOH X 1 mol NaOH X 1 mol H 2 SO 4 = 0.250 mol H 2 SO 4 39.99 g NaOH 2 mol NaOH 27.6 g NaOH X 1 mol NaOH X 1 mol Na 2 SO 4 X 142.04 g Na 2 SO 4 = 49.0 g Na 2 SO 4 39.99 g NaOH 2mol NaOH 1 mol Na 2 SO 4

2AgNO 3(aq) + CaCl 2(aq) --> Ca(NO 3 ) 2(aq) + 2AgCl (s) 1.If you use 30.0 mL of 2.00 M CaCl2 solution, how many mL of 1.50 M AgNO3 need to be added to make the reaction go to completion? 2.If you use 50.0 mL of 2.00 M CaCl 2 and 30.0 mL of AgNO 3 how many grams of solid AgCl will be collected at the end? (remember limiting reactant)

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