At 0°C and 1.00 atm, as much as 0.84 g of O₂ can dissolve in 1.0 L of water. At 0°C and 4.00 atm, how many grams of O₂ dissolve in 1.0 L of water?

The Henry's law constant for helium gas in water at 30°C is 0.000370 M/atm. When the partial pressure of helium above a sample is 0.400 atm, what is the concentration of helium in the water?

What is the millimolar solubility of oxygen gas, O2, in water at 16 °C, if the pressure of oxygen is 1.00 atm? Express the millimolar concentration numerically to two significant figures.

What volume of water, in mL, is needed to dissolve 6.3×10^1 mg of carbon monoxide gas (28.0 g/mol) when the partial pressure of carbon monoxide above the water is 3.8 atm at 25 °C? The Henry's constant for carbon monoxide gas in water at 25 °C is 9.5×10^-1 M/atm.

What would be the vapor pressure at 25.0 °C of a solution of 5.00 g of glucose (C₆H₁₂O₆) in 100.0 g of ethanol (C₂H₅OH)? Pure ethanol has a vapor pressure of 54.68 mmHg at 25 °C.

At 25 °C, the solubility of O₂ is 4.55 × 10⁻³ M at 3.5 atm pressure. What is the solubility of O₂ at the same temperature and at 2.0 atm pressure?

A scuba diver is breathing compressed air that is 21% (by volume) oxygen at a depth of 66 ft. beneath the surface. The total pressure at this depth is 3.0 atm. The Henry's law constant (k) for O2 in water at a normal body temperature (37 °C ) is 1.93 * 10-3 mol>(L atm). What is the solubility of O2 in the blood of the diver at 66 ft. beneath the surface? (LO 13.9) (a) 1.22 * 10-3 M (b) 2.76 * 10-2 M (c) 1.22 * 10-1 M (d) 2.76 * 10-1 M