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Mass to Mass Stoichiometry grams of what you have g A moles of what you have mol A moles of what you want mol B grams of what you want g B Grams Moles Moles Grams

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Example #1 grams of what you have 30 g CH4 moles of what you have mol CH4 moles of what you want mol H2O grams of what you want g H2O 30 g CH 4 mol CH 4 mol H 2 O g H 2 O

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Example #1 CH 4 + 2O 2 CO 2 + 2H 2 O You have 30 g CH 4 that you burn in oxygen. How many grams of water (H 2 O) can you make? 30 grams CH 4 x 1 mole CH 4 = moles CH 4 16 grams moles CH 4 x 2 mole H 2 O = 3.75 moles H 2 O 1 mole CH moles H 2 O x 18 grams = 67.5 grams H 2 O 1 mole H 2 O

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Percent Yield Percent yield is a comparison if the amount of product actually produced in a reaction versus the theoretical amount calculated. Percent Yield = actual x 100 theoretical When the reaction in example 1 was performed, only 52 grams of H2O were produced. Calculate the percent yield.

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Baking Soda and Vinegar Volcano Congratulations on being ready to perform your experiment!

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Step 1 You will be given 5 g of vinegar (C 2 H 4 O 2 ). Calculate how many grams of baking soda (NaHCO 3 ) you need. C 2 H 4 O 2 + NaHCO 3 CO 2 + Na 2 CO 3 + H 2 O The equation is already balanced!

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Step 2 Calculate how many grams of water (H 2 O)you will make with your 5 g of vinegar (C 2 H 4 O 2 ). C 2 H 4 O 2 + NaHCO 3 CO 2 + Na 2 CO 3 + H 2 O The equation is already balanced!

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Step 3 Measure out baking soda and vinegar; mix in beaker. Measure empty container. Filter out Na 2 CO 3, so that water is in container. Measure mass of container and water to determine how much water you made.

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Percent Yield Calculate the percent yield of water produced by your reaction using the formula: Percent Yield = actual x 100 theoretical

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