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A bottle of fizzy water is sealed with carbon dioxide at a pressure of 3.0 bar at 298 K…

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A bottle of fizzy water is sealed with carbon dioxide at a pressure of $3.0\ \text{bar}$ at $298\ \text{K}$ . The Henry's law constant of carbon dioxide in water is $1.67\ \text{kbar}$ . How many grams of carbon dioxide ( $44\ \text{g/mol}$ ) dissolve in $1.00\ \text{kg}$ of water? The bottle is opened and left in the open air for a long time, where the partial pressure of carbon dioxide is $0.00040\ \text{bar}$ . How many grams stay in the water?

Need a reminder? The key ideaShow

Henry's law: $p = K_H\, x$ , where $x$ is the mole fraction of the gas in the solution. $K_H$ has the unit of pressure, and a larger $K_H$ means a smaller solubility. In a weak water solution, the moles of gas in $1\ \text{kg}$ of water are $x \times 55.6\ \text{mol}$ . Heating lowers the solubility of a gas.

The worked solution

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← Air has 21 % oxygen by volume. In a pond at 303 K, the Henry's law constant of oxygen is 46.82 kbar…A deep diver breathes a mixture of 80 % helium and 20 % oxygen by moles, at a total pressure of 5.0… →

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