Question

1) An alternative carbonation in beverages is nitrogenation (think nitro-brewed coffee). In class we used Henry's Law to calculate the amount of CO2 dissolved in water at T = 25°C and P = 5 bar. Find the mass of CO2 in a standard 12oz. can of carbonated water. What would the pressure need to be to dissolve the same mass of nitrogen in water at T = 25°C? What does this say about the amount of nitrogen in standard nitrogenated beverages? Useful data: A standard 12oz. beverage can has a mass of -355 g. Henry's constant for nitrogen in water at T = 25°C is H = 87650 bar

Answer 1

Since at T= 25°c = 298k tenay constant for Cozus Kri= 164.8.1618 bar Babel and Many pl Waton = 120p. - 3559 = Witzo Since quien P = Sbor cc KH, Taus assurning - 1780V Niquid phase will be opene water and Vapan phase will be fure Co2 Applying themy's law, Mole fraction of a CO2 in watch 24 1x Sbai 1648.1618 bar Kri Г. - - 162 Nozt n Hoo - 3-033x10-3 NHO = 329.6323 noz Wazo x 44 gnul = 328.6323 . 18 quel . 355 ax R2 x - 328.6323 a Woo W co.z) dirsowed = 8.64 g 2-64g of Eur-is diss. dved us hor at geven Cond. This

Now to cursolue 2.64 g of Nz in 1208. Nitrogenate drink WnZ Mode fraction of N₂ = 14x2 WN2 + 355 14x2 18 - 264 / 1 482 = 4675B x 10 46758 - -------- 2:64 355 14x2 18 - Kaze 4.758X60-3 Henry low with same assumption that Gan fhose will be purez de yo no 1 a yo x P = XNz x (keino a oxP = 4.453x1053 X 87650 bar PE 1117.033 bar z Thun 47.033 bar is required for the same