Breathing air that contains 4.0 % by volume CO2 over time
causes ...

Question

Breathing air that contains 4.0 % by volume CO2 over time
causes rapid breathing, throbbing headache, and nausea,
among other symptoms. What is the concentration of CO2
in such air in terms of (b) molarity, assuming 1 atm pressure and a body temperature of 37 °C?

Accepted Answer

Hi everyone for this problem, we're told to calculate the molar itty of 02 in the air which is 6% by volume at 1 80 M and 30 degrees Celsius. So our goal here is to calculate malaria T. Since we're dealing with gasses, the equation that we're going to use to solve this is the malaria T of 02 is going to equal the pressure of 02 over R times T. Okay, so we know what our is. It's r universal gas constant and we know what the temperature is but we don't know what the pressure of 02 is. In order for us to solve for the pressure of 02, it's going to be our pressure of 02 is equal to our mole fraction of 02 times our total pressure. Okay, we know what our total pressure is. It's 1 80 M. But what is our mole fraction? Since we are for gasses at the same temperature and pressure? The mole fraction and the volume fraction are the same. So we know that our volume fraction is 6%. So that means our mole fraction is going to be the same. Same. Okay, so when we plug that in our mole fraction we're going to convert that 6% to a decimal. So it's going to be 0.6 and our total pressure is 1 80 M. So that means our pressure of 02 is going to be 0.6 A T M. Okay, So now we can plug that in. So we get our pressure of 02 is 0.6 80 M. Over. R is a universal constant that we should know. That is 0.8 to 06 Leaders times atmosphere or a T. M. Over more times kelvin. And our temperature, they gave us our temperature and°C. But if we look at our our constant, our temperature is in Kelvin. So we need to convert that C to Kelvin. So to do that, we have 30°C, we're going to add 273.15. And when we do that we'll get our temperature in Kelvin. So that will be 303.15 Kelvin. Okay, so now we have everything to solve for Armel arat E. Okay, so let me um highlight that. And so when we do this calculation, we're going to get a final answer of 2.4 times 10 to the -3 molar. Okay. And that's our mill arat E. That's the end of this problem. I hope this was helpful

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