The value of Henry's constant for CO2 gas dissolved in water at 290 K is 12.8 MPa. Consider wate

step 1 Question number 117. The solution is obtained from the Henry's Law, where the pressure of the ca

The value of Henry's constant for CO2 gas dissolved in water...

The value of Henry's constant for $\mathrm{CO}_{2}$ gas dissolved in water at $290 \mathrm{K}$ is $12.8 \mathrm{MPa}$. Consider water exposed to atmospheric air at 100 kPa that contains 3 percent $\mathrm{CO}_{2}$ by volume. Under phase equilibrium conditions, the mole fraction of $\mathrm{CO}_{2}$ gas dissolved in water at $290 \mathrm{K}$ is $(a) 2.3 \times 10^{-4}$ $(b) 3.0 \times 10^{-4}$ $(c) 0.80 \times 10^{-4}$ $(d) 2.2 \times 10^{-4}$ $(e) 5.6 \times 10^{-4}$

The value of Henry's constant for $\mathrm{CO}_{2}$ gas dissolved in water at $290 \mathrm{K}$ is $12.8 \mathrm{MPa}$. Consider water exposed to atmospheric air at 100 kPa that contains 3 percent $\mathrm{CO}_{2}$ by volume. Under phase equilibrium conditions, the mole fraction of $\mathrm{CO}_{2}$ gas dissolved in water at $290 \mathrm{K}$ is
$(a) 2.3 \times 10^{-4}$
$(b) 3.0 \times 10^{-4}$
$(c) 0.80 \times 10^{-4}$
$(d) 2.2 \times 10^{-4}$
$(e) 5.6 \times 10^{-4}$

Key Concepts

Henry's Law

Henry's Law states that the amount of gas that dissolves in a liquid at a given temperature is directly proportional to the partial pressure of the gas in contact with the liquid. This principle is crucial in understanding and predicting the behavior of gaseous solutes in solvents under varying pressure conditions.

Henry's Constant

Henry's constant is the proportionality factor in Henry's Law that relates the solubility (often expressed as mole fraction) of a gas in a liquid to the partial pressure of the gas. It is temperature-dependent and specific to the gas-liquid pair, serving as a key metric in applications such as gas absorption and environmental chemistry.

Partial Pressure

Partial pressure is the pressure that a single component of a gas mixture would exert if it occupied the entire volume of the mixture alone. Understanding partial pressure is essential in applying Henry's Law, as it is used to determine the effective pressure driving the dissolution of each gas in a solvent.

Mole Fraction

Mole fraction is a way of expressing the concentration of a component in a mixture, calculated as the number of moles of that component divided by the total number of moles in the mixture. It is a dimensionless quantity that is particularly useful in the context of solutions and gas mixtures, especially when relating solubility to partial pressures in Henry's Law.

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