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Mass-Mass Stoichiometry

Mass-Mass Stoichiometry. If the mass of any reactant or product is known for a chemical reaction, it is possible to calculate the mass of the other reactants and products. Sample Problem: How many grams of carbon dioxide (CO 2 )

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Mass-Mass Stoichiometry

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  1. Mass-Mass Stoichiometry If the mass of any reactant or product is known for a chemical reaction, it is possible to calculate the mass of the other reactants and products.

  2. Sample Problem: How many grams of carbon dioxide (CO2) would be produced by the combustion of butane (C4H10) with 17.9 grams of oxygen (O2) as shown in the following chemical equation? 17.9 g ? 7 4 6 C4H12 + O2→ CO2 + H2O Step 1: Balance the chemical equation Note: Write the value of the given substance over that substance and put a “?” over the required substance. Ignore everything else in the equation

  3. 17.9 g? C4H12 + 7O2→ 4CO2 + 6H2O The solving process involves the use of dimensional analysis Step 2: Convert grams of given substance to moles 17.9 g O2 1 mol O2 32.0 g O2 4 mol CO2 7 mol O2 44.0 g CO2 1 mol CO2 = 28.1 g CO2 Step 3: Give ratio of moles required substance/given substance Step 4: Convert moles of required substance to grams Step 5: Cancel and solve

  4. Practice Problems Try to work the next problems on the paper first. Then use the power point to check your work.

  5. Practice Problem 1: What amount of barium chloride (BaCl2) would be made by the reaction of 105 g of hydrochloric acid (HCl) with barium nitrate as the following equation shows? 105 g? 2HCl + Ba(NO3)2 2HNO3 + BaCl2 Solve the above problem and check your answer below: 105.0 g HCl 1 mol HCl 36.5 g HCl 1 mol BaCl2 2 mol HCl 208 g BaCl2 1 mol BaCl2 = 299.2 g BaCl2

  6. Practice Problem 2: What amount of hydrogen (H2) must react with 13.3 g oxygen (O2) to completely consume the available oxygen and form water? ? 13.3 g 2H2 + O2 2H2O Solve the problem and then check your answer below. 13.3 g O2 1 mol O2 32 g O2 2 mol H2 1 mol O2 2.02 g H2 1 mol H2 = 1.68 g H2

  7. Practice Problem 3: How much sulfuric acid (H2SO4) is required to produce 31.2 grams of silver sulfate (Ag2SO4)? ?31.2 H2SO4 + 2AgCl Ag2SO4 + 2HCl Solve the problem and then check your answer below. 1 mol H2SO4 1 mol Ag2SO4 31.2 g Ag2SO4 1 mol Ag2SO4 312 g Ag2SO4 98.1 g H2SO4 1 mol H2SO4 = 9.81 g H2SO4

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