Henry's law constant (mol/L · atm) for oxygen dissolving in blood is 3.74 $\times$ 10^-2 mol/L · atm at body temperature, 37 $\circ$ 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. A)7.8 10^-3 M B)3.5 10^-3 M C)2.3 10^-2 M D)1.3 10^-2 M E)0.11 M

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The Answer of Henry's law constant (mol/L · atm) for oxygen dissolving in blood is 3.74 $\times$ 10^-2 mol/L · atm at body temperature, 37 $\circ$ 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. A)7.8 10^-3 M B)3.5 10^-3 M C)2.3 10^-2 M D)1.3 10^-2 M E)0.11 M

Henry's Law Constant (Mol/L · Atm) for Oxygen Dissolving in Blood