Breathing air that contains 4.0 by volume co2

Asked by maham237 @ 26/04/2021 in Chemistry viewed by 313 People

over time causes rapid breathing, throbbing headache, and nausea, among other symptoms. You may want to reference (Pages 539 - 541) Section 13.4 while completing this problem. Part A What is the concentration of CO2 in such air in terms of molarity, assuming 1 atm pressure and a body temperature of 37 ∘C? Express you

Answered by maham237 @ 26/04/2021

Answer:

$1.6x10^{-4}M$

Explanation:

Hello,

By volume percentage for this case is defined as:

$v/v=\frac{V_{CO_2}}{V}*100$

Since we've got a 4.0%by volume solution, it is related, for instance, with 4L of carbon dioxide per 100L of air, so the moles are computed via the ideal gas equation as:

$n_{CO_2}=\frac{PV}{RT}=\frac{1atm*4L}{0.082\frac{atm*L}{mol*K}*310K} \\n_{CO_2}=0.16molCO_2$

Finally, applying the molarity formula we get:

$M=\frac{n_{CO_2}}{V} =\frac{0.16mol}{100L}=1.6x10^{-4}M$

Best regards.

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