The Henry\'s Law constant at 25 degree C for carbon dioxide gas(44.01 g/mole) in

Question

The Henry's Law constant at 25 degree C for carbon dioxide gas(44.01 g/mole) in water is 0.034 M/atm. A can of coke contains 355 mL of liquid (assume water) and 2.2g dissolved CO_2. Use this information to answer questions 28 -30. ___Calculate the pressure (atm) of CO_2 required to dissolve this quantity of CO_2. At 25 degree C. A) 4.1 atm B) 0.41 atm C) 0.0048 atm D) ___If the coke solution is prepared at a temperature below 25 degree C, the pressure of CO_2 required to again dissolve 2.2 g CO_2 in 355 mL of solution would be ___ the pressure that was required at 25 degree C. A) greater than B) less than C) equal to D) insufficient information ___Immediately after a coke can is opened, the CO_2 solution inside is A) unsaturated B) saturated C) supersaturated D) insufficient information

Explanation / Answer

31]

Solubility [S] = kH *Pressure

Solubility = 2.2 / 355*10^-3 = 6.197 gm/L

Convert it into moles/litre M = 6.197 / 44 = 0.14 M [MW of CO2 = 44]

S = kH*P

0.14 = 0.034*P

P = 4.14 atm

Answer is A

b]

PV = nRT

P is proportional to T at Constant V

P1 / P2 = T1 / T2

Since Temperature is decreases ...Pressure also decreases

Answer is B

33]

Assuming our 2.2 grams of carbon dioxide is the maximum amount of carbon dioxide that can be placed inside, some of the carbon dioxide is soluble in water while the rest exerts pressure inside the headspace to force the carbon dioxide inside the liquid. The pressure is necessary inside this closed volume as, once you open the cap, the carbon dioxide tries to achieve equilibrium.

CO2 (solution)CO2(g)

It is a supersaturated solution as more amount of CO2 is dissolved

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