Question
Use Henry's law to determine the molar solubility of helium at a pressure of 1.0 atm and $25^{\circ} \mathrm{C}$.
Step 1
Mathematically, it can be written as: C = kH * P where C is the molar concentration of the gas in the liquid, kH is the Henry's Law constant, and P is the partial pressure of the gas. Show more…
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Use Henry"s law to determine the molar solubility of helium at a pressure of 1.0 atm and 25 C.
Use Henry's law to determine the molar solubility of helium at a pressure of 1.4 atm and 25°C. Henry's law constant for helium gas in water at 25°C is 3.70 x 10^-4 M/atm.
The Henry's law constant for the solubility of helium gas in water is $3.8 \times 10^{-4}$ M/atm at $25^{\circ} \mathrm{C}$. (a) Express the constant for the solubility of helium gas in $\mathrm{M} / \mathrm{mm} \mathrm{Hg}$. (b) If the partial pressure of He at $25^{\circ} \mathrm{C}$ is $293 \mathrm{~mm} \mathrm{Hg}$, what is the concentration of dissolved He in $\mathrm{mol} / \mathrm{L}$ at $25^{\circ} \mathrm{C}$ ? (c) What volume of helium gas can be dissolved in $10.00 \mathrm{~L}$ of water at $293 \mathrm{~mm} \mathrm{Hg}$ and $25^{\circ} \mathrm{C} ?$ (Ignore the partial pressure of water.)
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