Stoichiometry Lab Report

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I. Purpose
We did this experiment to learn how to use stoiciometry with the ideal gas law to figure out the amounts of substances within a compound.
II. Hypothesis
If I measure the circumference of a balloon filled with gas and use it to determine the volume of gas, then I can use the ideal gas equation to find the number of moles of gas it contains.
III. Procedure
First we rinsed a 2-liter bottle with tap water. Then we measured out 200.0 g of white vinegar into the bottle using a mass scale and a funnel. Meanwhile, we measured out at least 30.0 g of baking soda into a balloon using another mass scale. We attached the balloon to the neck of the bottle, making sure it was completely attached with an airtight seal. We held up the balloon, letting the baking soda fall into the vinegar. After swirling the bottle around to make sure all of the baking soda reacted with the vinegar, we measured the circumference of the now-inflated balloon with a seamstress' tape measure. Finally, we cleaned up after doing some calculations.
IV. …show more content…

Data and Observations
Circumference: 57.50 cm = 5.750 dm
Radius = 5.750 dm ÷ 2π = 0.916 dm
V = 4/3πr3 = 4/3π(0.916 dm)3 = 3.22 dm3 = 3.22 L
Troom = 23.0 C so water vapor pressure = 21.1 torr = 0.0278 atm pressure of CO2 = total pressure - water vapor pressure = 1.003296 atm - 0.0278 atm = 0.975 atm
Tcarbon dioxide = 23.0 C = 296.0 K
Ideal Gas Law: PV = nRT n = PV ÷ RT = (0.975 atm)(3.22 L) ÷ (0.0821 L x atm/mole x K)(296.2 K) = 0.129 moles CO2
1 mole CO2 = 1 mole acetic acid, so 0.129 moles CO2 = 0.129 moles acetic

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