At 20^∘ C(293 K) and a partial pressure of 10^5 Pa, the solubility of CO2 in water is 0.169 g

step 1 Hi, so in this question we are asked the solubility of CO2 at the given temperature. So first of

At 20^∘ C(293 K) and a partial pressure of 10^5 Pa, the...

At $20^{\circ} \mathrm{C}(293 \mathrm{~K})$ and a partial pressure of $10^{5} \mathrm{~Pa}$, the solubility of $\mathrm{CO}_{2}$ in water is $0.169 \mathrm{~g} / 100 \mathrm{~mL}$. What is the solubility of $\mathrm{CO}_{2}$ at $33.3 \times 10^{5} \mathrm{~Pa}$ ?

Key Concepts

Henry's Law

Henry's law is a principle in physical chemistry that establishes a direct proportionality between the concentration of a gas dissolved in a liquid and the partial pressure of that gas above the liquid. This relationship, typically expressed as C = k_H * P, is vital for predicting how changes in pressure affect the solubility of gases in solvents.

Partial Pressure

Partial pressure refers to the individual pressure contributed by a single gas in a mixture of gases. In the context of gas solubility, it is the driving factor determined by the gas's pressure above a liquid that influences how much of the gas will dissolve, in accordance with Henry's law.

Gas Solubility

Gas solubility describes the extent to which a gas can dissolve in a liquid at a given temperature and pressure. It is crucial in various applications ranging from environmental science to industrial processes. The solubility is directly affected by the partial pressure of the gas and inversely affected by temperature, among other factors.

Unit Conversion

Unit conversion is an essential process in solving quantitative problems in chemistry to ensure that measurements such as mass, volume, and pressure are consistently used. Accurate conversion enables the correct application of principles like Henry's law when calculating the solubility of gases under varying conditions.

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