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# 4.08 Percent Yield Lab

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## taylor balcom

on 16 November 2015

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#### Transcript of 4.08 Percent Yield Lab

If you had not heated the product long enough to remove all of the water, explain in detail how that would have specifically affected your calculated actual yield and percent yield.
Create a data table to record your data from the procedure. Be sure that the data table is neat and organized and that all measurements have the correct significant figures and units.
Evaporating Dish: 24.35g
Evaporating Dish & NaHCO3 + HCl: 40.08g
Evaporating Dish & NaHCO3: 37.08g
Evaporating Dish & Salt Product: 31.52g
Write the complete balanced equation for the reaction that occurred in this lab. Hint: H2CO3 is not a final product of the double-replacement reaction; it breaks down (decomposes) immediately into two products.

Determine the percent yield of NaCl in your experiment, showing all work neatly in the space below.
The NaHCO3 is the limiting reactant and the HCl is the excess reactant in this experiment. Determine the theoretical yield of the NaCl product, showing all of your work in the space below.
What is the actual yield of NaCl in your experiment? Show your work below.
4.08 Percent Yield Lab
NaHCO3+HCl = CO2+H20+NaCl
31.52g-24.35g=7.14g NaCl
7.17g / 8.420g = 81090251 x 100 = 81%
If I had not heated the salt product long enough to remove all the water, the yield would increase, changing the calculations for the percent. If all the water had not evaporated, the weight of the dish would be greater.
37.08g-24.35g=12.73g NaHCO3
12.73g/84.01g mol= 0.152 mol NaHCO3
8.883g NaCl
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