The partial pressure of carbon dioxide gas inside a bottle of cola is 4.00 atm at 25 ° C. What is solubility of CO₂ at this temperature if k_H(CO₂) = 3.3×10^{- 2} M/atm?

Question

Quizplus · Accepted Answer

According to Henry's Law, the solubility (S) of a gas in a liquid is directly proportional to the partial pressure (P) of the gas above the liquid, with the constant of proportionality being the Henry's law constant (k). So, we can use the equation: P = kS Rearranging the equation, we get: S = P/k Here, the partial pressure of CO2 gas (P) is given as 4.00 atm. And, the Henry's law constant (k) for CO₂ at 25 °C is given as 3.3×10^{- 2} M/atm. So, substituting the values in the equation, we get: S = 4.00 atm / 3.3×10^{- 2} M/atm S = 0.121 M Therefore, the solubility of CO₂ in the cola at 25°C is 0.13 M (rounded to two significant figures). Hence, the best choice is B.

The Partial Pressure of Carbon Dioxide Gas Inside a Bottle