Mass-Mass Conversions 56.0 g N 2 x g N 2 g NH 3 28.0 1 1 2 = 1904 = 68.0 1. When nitrogen and hydrogen react, they form ammonia gas, which has the formula.

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Presentation transcript:

Mass-Mass Conversions 56.0 g N 2 x g N 2 g NH = 1904 = When nitrogen and hydrogen react, they form ammonia gas, which has the formula NH 3. If 56.0 g of nitrogen are used up in the reaction, how many grams of ammonia will be produced? N H 2  2 NH 3 mol N 2 x mol NH 3 x

Mass-Mass Conversions 42.0 g Na 2 O x g Na 2 O g Na = 3864 = Sodium metal reacts with oxygen to produce solid sodium oxide. How many grams of sodium must react to produce 42.0 g of sodium oxide? 2. Sodium metal reacts with oxygen to produce solid sodium oxide. How many grams of sodium must react to produce 42.0 g of sodium oxide? 4Na + O 2  2 Na 2 O mol Na 2 O x mol Na x

Mass-Mass Conversions 12.0 g H 2 x g H 2 g H 2 O = 216 = When 12.0 g of hydrogen reacts with oxygen, how many grams of water are produced? 2H 2 + O 2  2 H 2 O mol H 2 x mol H 2 O x

% Yield: Actual Yield: amount of product produced when the reaction is performed in a lab. Theoretical Yield: amount of product expected to be produced based on the balanced equation and the amount of reactants. Percent Yield = ( Actual yield / Theoretical yield) x 100%

% Yield 5.99 g C 3 H 8 x g C 3 H 8 g CO = = What is the % yield of carbon dioxide when 5.99 grams of propane are burned and grams of carbon dioxide are collected? C 3 H 8 + 5O 2  3CO 2 + 4H 2 O mol C 3 H 8 x mol CO 2 x Theoretical yield Actual yield

% Yield = Theoretical g CO = = What is the % yield of carbon dioxide when 5.99 grams of propane are burned and grams of carbon dioxide are collected? C 3 H 8 + 5O 2  3CO 2 + 4H 2 O Actual x 100 % = Theoretical yield Actual yield = g CO 2 x 100 % 67.0 %

Limiting and Excess Reagent Limiting Reactant Reactant used up first in a chemical reaction. (Limits amount of product produced!!) Excess Reactant Reactant that is not used up in a chemical reaction (Will have leftover reactant, too much!!)