The atmospheric pressure in a lab is calculated as 1.3 atm. If oxygen gas contributes 62% of this atmospheric pressure, determine its mass (in g) dissolved at room temperature in 25 L of water. The Henry's Law Constant for oxygen in water at this temperature is 5.3 × 10^–5 M/atm.

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 solubilityof 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

Fish generally need an O2 concentration in water of at least 4 mg/L for survival. What partial pressure of oxygen above the water in atmospheres at 0 °C is needed to obtain this concentration? The solubility of O2 in water at 0 °C and 1 atm partial pressure is 2.21 * 10-3 mol>L.