The solubility of CO2 gas in water is 0.15 g / 100 mL at a CO2 pressure of 101,325 Pa. (a) Wh

step 1 Looking at the first part of this question, we need to recall that the solubility of CO2 can be

The solubility of CO2 gas in water is 0.15 g / 100 mL at a...

The solubility of $\mathrm{CO}_{2}$ gas in water is $0.15 \mathrm{~g} / 100 \mathrm{~mL}$ at a $\mathrm{CO}_{2}$ pressure of $101,325 \mathrm{~Pa}$. (a) What is the solubility of $\mathrm{CO}_{2}$ in a soft drink (which is mainly water) that was bottled under a $\mathrm{CO}_{2}$ pressure of $4.6 \times 10^{5} \mathrm{~Pa} ?$ (b) An atmospheric concentration of $380 \mathrm{ppm}, \mathrm{CO}_{2}$ corresponds to a partial pressure of $38.5 \mathrm{~Pa}$. What percentage of the $\mathrm{CO}_{2}$ originally dissolved in the solution in part (a) remains in solution after the soft drink reaches equilibrium with the ambient atmosphere? (c) One bottle of soda is stored in a refrigerator at $3^{\circ} \mathrm{C}$ $(276 \mathrm{~K})$, and another is stored at room temperature $\left(25^{\circ} \mathrm{C}\right.$ or $\left.298 \mathrm{~K}\right)$. If both bottles are opened simultaneously, which one would exhibit greater carbonation (i.e., bubbles)? Explain.

The solubility of $\mathrm{CO}_{2}$ gas in water is $0.15 \mathrm{~g} / 100 \mathrm{~mL}$ at a $\mathrm{CO}_{2}$ pressure of $101,325 \mathrm{~Pa}$.
(a) What is the solubility of $\mathrm{CO}_{2}$ in a soft drink (which is mainly water) that was bottled under a $\mathrm{CO}_{2}$ pressure of $4.6 \times 10^{5} \mathrm{~Pa} ?$
(b) An atmospheric concentration of $380 \mathrm{ppm}, \mathrm{CO}_{2}$ corresponds to a partial pressure of $38.5 \mathrm{~Pa}$. What percentage of the $\mathrm{CO}_{2}$ originally dissolved in the solution in part (a) remains in solution after the soft drink reaches equilibrium with the ambient atmosphere?
(c) One bottle of soda is stored in a refrigerator at $3^{\circ} \mathrm{C}$ $(276 \mathrm{~K})$, and another is stored at room temperature $\left(25^{\circ} \mathrm{C}\right.$ or $\left.298 \mathrm{~K}\right)$. If both bottles are opened simultaneously, which one would exhibit greater carbonation (i.e., bubbles)? Explain.

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Key Concepts

Equilibrium in Gas-Liquid Systems

At equilibrium, the rate at which a gas dissolves into a liquid equals the rate at which it escapes. This dynamic balance ensures a constant concentration of dissolved gas under steady conditions, and any changes in pressure or temperature can shift this balance.

Temperature Dependence of Gas Solubility

Temperature affects gas solubility in liquids, where lower temperatures typically increase solubility and higher temperatures decrease it. This relationship is important because it explains how thermal changes alter the behavior of gases dissolved in a solution.

Gas Partial Pressure

Gas partial pressure refers to the pressure exerted individually by a component gas in a mixture. It plays a critical role in determining the concentration of a gas that dissolves in a liquid, as described by Henry’s Law.

Henry’s Law

Henry’s Law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid. This principle enables prediction of how varying pressures affect the amount of gas dissolved within a solution when temperature remains constant.

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