I wanted to drink Coca Cola so I filled up my water bottle
with the soda in Frank. When I went home, I put the water bottle in the
refrigerator and a few hours later, when I opened it, there was a lot of gas
released. Thus, I wanted to find the amount of gas released from the bottle. To
make the calculations easier, I assumed that when I opened the bottle, all the
gas that was in the liquid was released.

There are some unknowns that I had to search up online. There
is 2.2 grams of CO2 per 355 milliliters.

Thus, (2.2g CO2/355 mL) X (1000mL/1L) = 6.197 grams of CO2/L

(6.197g CO2/ 1L) X (1 mol CO2/ 44g CO2) = 0.1404 moles of CO2/1L

R= 0.082 L*atm/mols*K

Temperature in the fridge is 40 degrees
Fahrenheit

^{2}
40 degrees of Fahrenheit X (273.15K/ 32 degrees Fahrenheit)= 313.15K

The dimensions of the bottle are as
follows: 10.2 inches height and 2.5 inches in diameter

Volume is 80.11 inches

^{3 }= 2.035 meters^{3}= 1.313 liters^{3}
From these
measurements, I can find the pressure of the gas above the liquid.

PV= nRT

P= (nRT)/V

P= [(.1404 mol)(.082 L*atm/ mols*K)(313.15K)]/ 1.313 L

P= 2.746 atm^{3}
The
pressure of the gas molecules that escaped the liquid in the bottle is
calculated to be, 2.746 atm. Since the pressure of the atmosphere is 1 atm,
there was a release of gas from the bottle when it was opened.

References:

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