Dr BOB can you explain this to me. I am so struggling with this subject.
NO one has helped me on this one yet can anyone help me?
during a typical breathing cycle the CO2 concentration in the expired air rises to a peak of 4.6% by volume. Calculate the partial pressure of the CO2 at this point, assuming 1 bar of pressure. what is the molarity of the CO2 in the air at this point, assuming body temp is 37 degreesC.
To calculate the partial pressure of CO2 at the given concentration, we need to convert the percentage by volume to a partial pressure value. The partial pressure of a gas is the pressure it would exert if it occupied the same volume alone at the same temperature.
To convert the percentage by volume to partial pressure, we can use the Ideal Gas Law, which states:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature in Kelvin
First, let's convert the percentage to a decimal: 4.6% = 0.046
Since we know the total pressure is 1 bar, the partial pressure of the CO2, in bar units, can be calculated as:
Partial Pressure of CO2 = (percentage by volume / 100) * Total Pressure
Partial Pressure of CO2 = (0.046) * 1 bar = 0.046 bar
Now, let's calculate the molarity of CO2 in the air at this point.
Molarity is defined as the number of moles of solute (CO2 in this case) divided by the volume of the solution (air in this case) in liters.
To calculate molarity, we need to know the volume of the air. However, the given information does not provide the volume. Therefore, we cannot determine the molarity of CO2 without the volume of air.
I hope this explanation helps you understand how to approach the problem. If you have any further questions, please let me know!