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4.08 Percent Yield

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by

Rachelle Clerjeau

on 26 May 2015

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Transcript of 4.08 Percent Yield

2. 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. (3 points)
HCI + NaHOC3 ----> H20 + CO2 + NaCI
3. 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. (5 points)
37.06g - 24.35g (evaporating dish) = 12.71 g NaHCO3

since
1 mol NaHCO3 & 1 HCl --> 1 mol NaCl & 1 H2O & 1 CO2

12.71 g NaHCO3 and 58.44 g/mol NaCl / 84.01 g/mol NaHCO3 = 8.841 grams of NaCl

Determine the percent yield of NaCl in your experiment, showing all work neatly in the space below.
7.17/8.8420x100= 81%
What is the actual yield of NaCl in your experiment? Show your work below.
31.52g - 24.35g = 7.17
Thank you!
Data Table
Empty Dish: 24.35g
Dish with NaHCO3 - 37.07g
Dish after the reaction - 40.06g
Dish after water evaporate - 31.53g

4.08 Percent Yield
By Rachelle Clerjeau
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.
If I didn't heat up the product the percent yield would be higher and the actual yield itself.
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