Chapter_8 Oct_22 Lecture_27.pptx

# Loss due to glassware sticks to glassware reaction

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Loss due to glassware =sticks to glassware = reaction doesn’t work exactly right = evaporation of volatile product (gas) The percent yield tells what percentage the actual yield is of the theoretical yield. actual yield % yield = 100% theoretical yield

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6 Determining the Limiting Reactant (actually have 0.118 mol) Thus, HCl is excess reactant and Zn is limiting reactant. The yield of product based on the amount of limiting reactant limiting reactant
Determining the Limiting Reactant Synthesizing PCl 3 according to the following reaction: P(s) + Cl 2 (g) PCl 3 (l) Mix 12.0 g of P and 35.0 g Cl 2 How much PCl 3 is produced? L.R. is Cl 2 45.2 g of PCl 3 is produced

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Determining the Limiting Reactant
In the example above, suppose you measure the ACTUAL yield to be 42.4 g. What is the percent yield? Determining the Percent Yield

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The reaction of methane and water is one way to prepare hydrogen: CH 4 (g) + H 2 O (g) → CO 2 (g) + H 2 (g) If 995 g of CH 4 reacts with 2.510 x 10 3 g of water, how many moles of reactants and products are there when the reaction is finished? Determining the Limiting Reactant
Determining the Limiting Reactant

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Rest of Chapter 8 Will not be in exam 3…but too cool to avoid
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