Click to see additional instructions This question is for extra credit. BACKGROU

Question

Click to see additional instructions This question is for extra credit. BACKGROUUND: In units of atmospheres (atm), atmospheric pressure at sea level is 1 atm (equivalent to 760 mm Hg). The partial pressure of each gas in the atmosphere can be calculated by multiplying atmospheric pressure (1 atm) by the mole fractional concentration of that gas. For example, the partial pressure of O2 is 0.2095 atm (equivalent to 159 mm Hg). A similar calculation can be done for CO2, using its mole fractional concentration in the atmosphere. QUESTION: Using the partial pressures of O2 and CO2 in atmospheric air at sea level, expressed in units of atm, and the absorption coefficients for these gases, the concentrations of O2 and CO2 in distilled water at a temperature of 0 C can be calculated in units of mmol/L. When these calculations are done, the concentration of O2 is found to be mmol/L, and mmol/L. (Express your answer to the concentration of CO2 is found to be two decimal places.)

Explanation / Answer

As the Henry law is based on the atmospheric unit of pressure, to get the answer of this problem, you should go through the atm unit of the pressure.

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