**Fugacities in a Can of Soda**

The fugacities of water and carbon dioxide are calculated as a function of temperature for a closed container, which is a model of a can of soda. The concentrations of the two components are calculated in both the liquid and the gas phases. As the temperature increases, the pressure increases, and therefore the fugacities increase. Note that the CO_{2} concentration is much lower than the H_{2}O concentration in the liquid phase, but the CO_{2} concentration is much higher than the H_{2}O concentration in the gas phase. Because the gas phase is assumed to be ideal, the fugacities of CO_{2} and H_{2}O in both phases are equal to their gas-phase partial pressures, and thus the CO_{2} fugacity is much higher than the H_{2}O fugacity. As the temperature increases, the CO_{2} concentration in liquid water decreases. However, as the temperature increases, the pressure increases, and a higher CO_{2} pressure increases the CO_{2} concentration in water, so the net effect is that the concentration in the liquid phase does not change much as the temperature increases.
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