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4.08 Percent Yield - Chemistry
Transcript of 4.08 Percent Yield - Chemistry
Empty Dish - 24. 35g
Dish with NaHCO3 - 37.06g
Dish after reaction - 40.06g
Dish after H2O evaporated - 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. HCI + NaHCO3 ---> H20 + CO2 + NaCI 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. 12.71 g of NaHCO3 divided by 84.01 g/mol (molar mass of it) = 0.1513 moles
0.1513 moles of NaHCO3 being consumed = 0.1513 moles of NaCI produced. I then multiply 0.1513 moles by molar mass of NaCl giving us the answer of 8.8420 grams of NaCI which is the theoretical yield. What is the actual yield of NaCl in your experiment? Show your work below. 31.52 g - 24.35 g = 7.17 g ( Mass of NaCI after all water evaporated) Determine the percent yield of NaCl in your experiment, showing all work neatly in the space below. Determine the percent yield of NaCl in your experiment, showing all work neatly in the space below. 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. Actual Yield would increase.
The product will be heavier since it was not thoroughly dried.
Percent Yield would increase
Percent Yield = actual yield/theoretical yield x 100%
- the actual yield increases, therefore percent yield also increases since actual yield in the numerator.