What is the pressure of CO2 inside the wine bottle at 25 degrees celsius.?

Question

The reaction is C6H12O6 (aq) --> 2C2H5OH (aq) + 2CO2 (g).
Fermentation of 750 mL grape juice (density = 1 g/mL) is allowed to take place in a bottle with a total volume of 825 mL until 12% by volume is ethanol (C2H5OH). If CO2 is soluble in H2O (obeys Henry's Law), what would be the pressure of CO2 inside the wine bottle at 25 degrees C? at 125 degrees C? Use the data given in the problem to calculate the partial pressure of CO2 in the gas phase and the solubility of CO2 in the wine at 25 degress C. The Henry's law constant for CO2 is 3.1 x 10^ -2 mol/L . atm at 25 C with Henry's law in the form C = kP, where C is the concentration of the gas in mol/L.
This question is really confusing..can someone help me please?

Answer 1

The previous answer is quite correct. Here is a bit more help.

You can find out the total number of moles CO2 from the balanced equation and the total number of moles of ethanol formed.

Let the pressure inside the bottle be P.

Then you have, from the gas law, n(gas) = P x 0.075 L/RT
And from Henry's Law, n(solution) = 3.1 x 10^-2 x P x 0.75 L

Add these up, put them equal to the total moles CO2 formed, and you have a simple equation in P.

Answer 2

You can calculate the number of moles of CO2 produced with the usual methods. Then it's time for some algebra; some of the CO2 will be gaseous (call it x), and the rest will be in solution. The Henry's law constant, which is given, will permit establishing a relationship involving x, and the gas law, applied to the 75 milliliters not full of booze will give you another. But there is no way of calculating anything at 125 C, as the solubility constant will be different at that temperature.