A common antacid tablet usually contains 2.0 g of sodium hydrogen carbonate (NaHCO3). Using this value, show how your carbon dioxide result compares with the theoretical values.
I can't compare what you didn't post.
Balloon No./Amount of Antacid /Amount/Balloon circumference
1 / 1 tablet / 5ml of Water(ml)/balloon after 10mins/after 20mins
2 / 2 tablets / 5ml / /
3 / 3 tablets / 5ml / /
/The volume of balloon/
NOTE: Use the maximum circumference of each balloon to calculate the volume of each balloon. Assume the balloon is spherical.
A common antacid tablet usually contains 2.0 g of sodium hydrogen carbonate (NaHCO3). Using this value, show how your carbon dioxide result compares with the theoretical values.
If you posted any data that allows us to calculate the volume of the balloon, I don't see it.
I don't know what experiment you're doing but I assume you added some acid to make the NaHCO3 decompose. You might try post the experiment and the data to see if we can make sense of it.
1. Cut an antacid tablet into small pieces and put them into an empty and round balloon. Do the same to the two tablets of antacid and place them into a second balloon. Repeat using three tablets and a third balloon.
2. Place 5 mL of water in the first balloon and immediately tie a knot at the neck of the balloon. Do the same for the other two balloons. Shake the balloons to mix the contents.
3. Carefully measure and record the circumference of the balloons for the next 20 minutes. Use the maximum circumference of each balloon to calculate the volume of each balloon. Assume the balloon is spherical.
4. Tabulate the number of tablets and the volume of the balloon.
OK. Did you add acid to the balloons after adding the 5 mL water. If so, how much? Did the water contain an acid?
What was the circumference of balloon #1? #2? #3?
The reaction is NaHCO3 + HX ==> NaX + CO2 + H2O
For 2 grams of antacid of NaHCO3 you will have moles NaHCO3 = g/molar mass = 2.0/84 = 0.0238 for 1 tablet and balloon #1, 0.0238 x 2 = ? mols for two tablets and balloon #2 and 0.0238 x 3 = ? moles for three tablets and balloon #3.
So theoretical yield in L = 0.0238 moles CO2 for one tablet or 0 =.0238 x 22.4 L/mol = liters CO2 for one tablet and balloon #1. That will be 0.0238 x 2 x 22.4 L/mol for two tablets and balloon #2 or 0.0238 x 3 x 22.4 L/mol = ? L for three tablets and balloon #3.
Then take your measurements for circumference of balloon #1, balloon #2 and balloon #3. Determine the volume from volume sphere = (4/3)*pi*r^3 and compare the volume of each balloon with the theoretical yolume I calculated above. Note that when you get the diamaeter of the balloon (I would measure it in cm or convert the measurement to cm and 1000 cc = 1 L) you caculate radius from r = diameter/2
To compare the carbon dioxide (CO2) result with the theoretical values, we need to calculate the theoretical amount of CO2 that should be produced from the given amount of sodium hydrogen carbonate (NaHCO3).
The balanced chemical equation for the reaction between sodium hydrogen carbonate and an acid (such as hydrochloric acid) is as follows:
NaHCO3 + HCl → NaCl + H2O + CO2
From the equation, we can see that 1 mole of NaHCO3 reacts to produce 1 mole of CO2.
First, we need to calculate the number of moles of NaHCO3 in 2.0 g. The molar mass of NaHCO3 can be calculated by adding the atomic masses of each element:
Na: 23.0 g/mol
H: 1.0 g/mol
C: 12.0 g/mol
O: 16.0 g/mol (three of them)
So, the molar mass of NaHCO3 is:
(1 x 23.0 g/mol) + (1 x 1.0 g/mol) + (1 x 12.0 g/mol) + (3 x 16.0 g/mol) = 84.0 g/mol
To calculate the number of moles, we use the formula:
moles = mass / molar mass
moles of NaHCO3 = 2.0 g / 84.0 g/mol = 0.024 moles
Since the balanced equation tells us that 1 mole of NaHCO3 produces 1 mole of CO2, the theoretical amount of CO2 produced is also 0.024 moles.
Now, to compare the experimental result with the theoretical values, you would need to provide the result of the actual amount of CO2 produced from the experiment. You can then compare this value with the theoretical value we calculated to determine the percentage difference or any deviations between them.