Yoloswag

04.08 Percent Yield: Percent Yield Lab Report and Rubric

1. 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. (3 points)

Mass of dish | Mass of dish after adding three scoops of NAHCO3 | Mass of dish after adding six drops of HCL | Mass of dish after evaporating the water |

24.35g | 37.06g | 40.06g | 31.52g |

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)

                                               NaHCO3 + HCl → NaCl + CO2 + H2O

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)

37.06 - 24.35 = 12.71 NaHCO3

12.71 NaHCO3 / 84.01 grams per mol = 0.1513

0.1513 * 58.4428 g/mol = 8.84239564

Theoretical yield = 8.84239564

4. What is the actual yield of NaCl in your experiment? Show your work below. (4 points)

31.52 - 24.35 = 7.14

Actual yield of NaCl = 7.14

5. Determine the percent yield of NaCl in your experiment, showing all work neatly in the space below. (5 points)

7.14 / 8.84239564 = 0.807

Percent yield = 81%

6. 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. (5 points)

If I had not heated the product long enough to remove all of the water, the actual yield and percent yield would have been affected because since there is water left over, the actual yield and percent yield would be higher and would be inaccurate.