4. (a) Normal air at earth\'s surface contains 0.350% CO2 by volume. What is the

Question

4. (a) Normal air at earth's surface contains 0.350% CO2 by volume. What is the partial pressure of CO2 in atm? b) The Henry's Law constant for CO2 dissolved in blood is 23.3 mM/atm. If the average person has 5.0L of blood, calculate the mass of CO2 dissolved in their blood (c) At the ocean's average depth of 3800m, the pressure is 378 atm. If a submarine (filled with normal air at the surface) were to equilibriate its internal pressure with the external pressure, what would be the partial pressure of CO2 at this depth?

Explanation / Answer

Part a

Total pressure at earth's surface = 1 atm

Mol fraction of CO2 = 0.350/100 = 0.0035

Partial pressure of CO2 = total pressure x Mol fraction of CO2

= 1 atm x 0.0035

= 0.0035 atm

Part b

Moles of CO2 = Henry's constant x volume x Pressure

= ( 23.3 x 10^-3 mol/L-atm) x( 5L) x 1 atm

= 0.1165 mol x 44 g/mol

= 5.126 g

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