Refer to Figure 11.10 . (a) How did the concentration of...

Refer to Figure $11.10 .$
(a) How did the concentration of dissolved $\mathrm{CO}_{2}$ in the beverage change when the bottle was opened?
(b) What caused this change?
(c) Is the beverage unsaturated, saturated, or supersaturated with $\mathrm{CO}_{2}$ ?

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Key Concepts

Henry’s Law

Henry’s Law governs the relationship between the concentration of a gas dissolved in a liquid and the partial pressure of that gas in the surrounding atmosphere. This principle explains that when the pressure above the liquid decreases, the solubility of the gas also decreases, causing the gas to escape from the solution.

Phase Equilibrium and Gas Solubility

Phase equilibrium refers to the balance between the dissolved gas in the liquid and the gas in the headspace. Changes in external conditions, such as pressure when a container is opened, disturb this equilibrium and alter the concentration of the dissolved gas as the system seeks a new balance.

Supersaturation

Supersaturation occurs when a liquid contains more dissolved gas than it would under equilibrium conditions at a given pressure. This state is common in closed systems that have been pressurized and then subsequently depressurized, leading to an excess of dissolved gas that can escape as bubbles once the pressure is released.

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