Question

Enter your answer in the provided box. The partial pressure of CO2 gas above the liquid in a bottle of champagne at 20°C is 4.5 atm. What is the solubility of CO2 in champagne? Assume the Henry's law constant is the same for champagne as it is for water: at 20°C, kH = 3.7 × 10−2 mol/(L·atm).

Answer 1

The solubility of CO2 in champagne at 20°C with a partial pressure of 4.5 atm is calculated using Henry's Law to be 0.1665 mol/L.

Step-by-step explanation:

The partial pressure of CO2 gas above the liquid in a bottle of champagne at 20°C is 4.5 atm, and we are given that the Henry's law constant at 20°C is 3.7 × 10−2 mol/(L·atm). To find the solubility of CO2 in champagne, we use Henry's Law, which states that the solubility of a gas in a liquid at a given temperature is proportional to the partial pressure of the gas above the liquid. The formula for Henry's Law is Sg = kH × Pg, where Sg is the solubility of the gas, kH is the Henry's law constant, and Pg is the partial pressure of the gas.

Using this formula, the solubility (Sg) can be calculated as follows:

Sg = (3.7 × 10−2 mol/(L·atm)) × (4.5 atm)

Sg = 0.1665 mol/L

Therefore, the solubility of CO2 in champagne at 20°C and a partial pressure of 4.5 atm is 0.1665 mol/L.

Answer 2

Answer: The molar solubility of carbon dioxide gas is 0.17 M

Step-by-step explanation:

Henry's law states that the amount of gas dissolved or molar solubility of gas is directly proportional to the partial pressure of the liquid.

To calculate the molar solubility, we use the equation given by Henry's law, which is:

`C_(CO_2)=K_H* p_(liquid)`

where,

`K_H` = Henry's constant =
`3.7* 10^(-2)mol/L.atm`

`p_(CO_2)` = partial pressure of carbonated drink = 4.5 atm

Putting values in above equation, we get:

`C_(CO_2)=3.7* 10^(-2)mol/L.atm* 4.5atm\\\\C_(CO_2)=0.17mol/L=0.17M`

Hence, the molar solubility of carbon dioxide gas is 0.17 M