Question

Reaction Run 3 Measured Mass of NaHCO3 = 0.99 g, Measured Mass of H3C6H5O7 = 1.52 g, Measured Mass of CO2 = 0.48 g. Determine the limiting reactant in the reaction run 3. Describe your reasoning. (10 points)

Calculate the amount (in g) of carbon dioxide from the amount of the limiting reactant that you used in the reaction run 3. The amount that you calculate is called the theoretical yield. Show all your work. (10 points)

The measured mass of carbon dioxide in the table is the actual yield of carbon dioxide for the reaction run 3. Calculate the percent yield of carbon dioxide in the reaction run 3. Show all your work. (10 points)

Answer 1

balanced equation :

H3C6H5O7 + 3 NaHCO3 ----------------> Na3C6H5O7 + 3 CO2 + 3 H2O

192.12 g         252 g                                                            132 g

1.52 g               0.99 g

192.12 g H3C6H5O7 --------------> 252 g NaHCO3

1.52 g H3C6H5O7 --------------->      ??

mass of NaHCO3 needed = 1.52 x 252 / 192.12 = 1.99 g

but we have on;y 0.99 g .so

limiting reagent is NaHCO3

2)

252 g NaHCO3 ---------------> 132 g CO2

0.99 g NaHCO3 ---------------> ?? CO2

mass of CO2 formed = 0.99 x 132 / 252

                                  = 0.519 g CO2

percent yield = (0.48 / 0.519 ) x 100

                      = 92.56 %