thugginwitnaeeLv1

20 May 2023

Data and Calculations (Part 1): include UNITS and show work where applicable.

1 tablet 2 tablets

(1) Measure the Circumference: (in centimeters)

(2) Calculate the radius of each balloon: (in cm)

r = circumference

2

(3) THEN, Convert the radius to dm (divide by 10)

(4) Calculate the volume of each sphere: (dm3)

V = 4r3

3

(5) Use the Ideal Gas Law to calculate # of moles (n):

(in moles)

PV = nRT

where P = 101.3 kPa

R = 8.31 (dm3 x kPa / mol x K) and T = 293 K.

(6) Calculate mass of CO2 (g) produced by multiplying

# of moles by its molar mass. (in grams)

Record in table below in Actual mass (Yield)

of CO2.

Calculations (Part 2):

(7) Refer to the balanced chemical equation for this reaction:

3NaHCO3(aq) + H3C6H7O7(aq) → Na3C6H7O7(aq) + 3CO2(g) + 3H2O(l)

Determine the mass of CO2(g) that can be formed from one tablet if it contains 1.9 grams of NaHCO3(s) and 1.0

grams of H3C6H7O7(s). Show your work below. Record this as your theoretical yield. (Hint: This is a limiting

reactant problem. The lowest mass is the MAX product.)

(8) Determine your percent yield for each reaction. Be sure to change the theoretical mass to 2 tablets

# of Tablets

Actual Mass (Yield) of

CO2(g)

(Answer from #6)

Theoretical Yield of CO2(g)

(calculated in #7)

Percent Yield of CO2(g)

% 𝒚𝒊𝒆𝒍𝒅 =

𝒂𝒄𝒕𝒖𝒂𝒍

𝒕𝒉𝒆𝒐𝒓𝒆𝒄𝒕𝒊𝒄𝒂𝒍 × 𝟏𝟎𝟎

Mass of 1

tablet =

Mass of 2

tablets =

(9) How does the Percent yield reflect the success or error of your experiment and suggest WHY it is not

what you expected?