4.08 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. (3 points) Events
Masses
Empty Dish
24.35 g
Dish with NaHCO3
37.06 g
Dish with NaHCO3 and HCI
40.06 g
Dish after burning
31.52 g
Write the complete balanced equation for the reaction that occurred in this lab. Hint: H2CO3 is not a final product of the doublereplacement reaction; it breaks down (decomposes) immediately into two products. (3 points) ___HCl___ + __NaHCO3___ → __H2O___ + __CO2___ +
__NACl___
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) 12.71 NaHCO3 / 84.01 g/mol = 0.1513 moles
0.1513 moles * 58.44 g/mol (NaCL molar mass) = 8.84197 g What is the actual yield of NaCl in your experiment? Show your work below. (4 points) 31.52 g 24.35 g = 7.17 g Determine the percent yield of NaCl in your experiment, showing all work neatly in the space below. (5 points) 7.17 g / 8.8197 g = 0.81295 = 81% 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) The product’s mass would be greater making the calculations adjust. If my actual yield is greater, then so would my percent yield.
Masses
Empty Dish
24.35 g
Dish with NaHCO3
37.06 g
Dish with NaHCO3 and HCI
40.06 g
Dish after burning
31.52 g
Write the complete balanced equation for the reaction that occurred in this lab. Hint: H2CO3 is not a final product of the doublereplacement reaction; it breaks down (decomposes) immediately into two products. (3 points) ___HCl___ + __NaHCO3___ → __H2O___ + __CO2___ +
__NACl___
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) 12.71 NaHCO3 / 84.01 g/mol = 0.1513 moles
0.1513 moles * 58.44 g/mol (NaCL molar mass) = 8.84197 g What is the actual yield of NaCl in your experiment? Show your work below. (4 points) 31.52 g 24.35 g = 7.17 g Determine the percent yield of NaCl in your experiment, showing all work neatly in the space below. (5 points) 7.17 g / 8.8197 g = 0.81295 = 81% 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) The product’s mass would be greater making the calculations adjust. If my actual yield is greater, then so would my percent yield.