The Henry's law constant for oxygen dissolving in blood is 3.74 *10^-2 mol/L . atm at body temperature, 37$\degree$C.Calculate the molar concentration of oxygen in blood for an alpine climber where the atmospheric pressure is 0.45 atm.The mole fraction of oxygen in air is 0.209.

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Henry's law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. The concentration of oxygen in blood can be calculated using the formula: $C = kP$, where $C$ is the concentration of the gas, $k$ is Henry's law constant, and $P$ is the partial pressure of the gas. Given that the Henry's law constant for oxygen in blood is $3.74 \times 10^{-3} \, \text{mol/L} \cdot \text{atm}$, and the partial pressure of oxygen is the product of the total atmospheric pressure and the mole fraction of oxygen in air ($0.45 \, \text{atm} \times 0.209$), the calculation is as follows:$$C = 3.74 \times 10^{-3} \, \text{mol/L} \cdot \text{atm} \times (0.45 \, \text{atm} \times 0.209) = 3.5 \times 10^{-4} \, \text{M}$$Therefore, the correct answer is $3.5 \times 10^{-4} \, \text{M}$, which corresponds to choice B.

The Henry's Law Constant for Oxygen Dissolving in Blood Is °\degree°

The Henry's Law Constant for Oxygen Dissolving in Blood Is $\degree$