During a person’s typical breathing cycle, the CO2 concentration in the expired air rises to a peak of 4.6% by volume. (b) What is the molarity of the CO2 in the expired air at its peak, assuming a body temperature of 37 °C?

Name: Chemistry: The Central Science
Author: Brown
ISBN: 9780134414232

Verified step by step guidance

Convert the percentage by volume of CO2 to a fraction by dividing by 100. This gives the volume fraction of CO2 in the expired air.

Use the ideal gas law, PV = nRT, to relate the volume fraction to molarity. Assume the pressure is 1 atm and convert the temperature from Celsius to Kelvin by adding 273.15 to 37 °C.

Calculate the volume of 1 mole of gas at 37 °C and 1 atm using the ideal gas law. This will give you the volume in liters that 1 mole of gas occupies under these conditions.

Determine the number of moles of CO2 in the expired air by multiplying the volume fraction of CO2 by the volume of 1 mole of gas calculated in the previous step.

Calculate the molarity of CO2 by dividing the number of moles of CO2 by the volume of the gas in liters. This will give you the molarity of CO2 in the expired air.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Molarity

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in moles per liter (mol/L) and is crucial for understanding how much of a substance is present in a given volume of solution. In this context, we need to calculate the molarity of CO2 in the expired air, which involves converting the percentage by volume into moles and then relating it to the volume of air.

Ideal Gas Law

The Ideal Gas Law is a fundamental equation in chemistry that relates the pressure, volume, temperature, and number of moles of a gas. It is expressed as PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin. This law allows us to calculate the number of moles of CO2 in the expired air based on its volume and temperature.

Body Temperature and Gas Behavior

Body temperature, typically around 37 °C, affects the behavior of gases, including their volume and pressure. When calculating gas concentrations, it is essential to convert the temperature to Kelvin (310 K) and consider how temperature influences gas properties. This understanding is necessary for accurately applying the Ideal Gas Law to determine the molarity of CO2 in the expired air.

Related Practice

Textbook 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?

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Textbook Question

Brass is a substitutional alloy consisting of a solution of copper and zinc. A particular sample of red brass consisting of 80.0 % Cu and 20.0 % Zn by mass has a density of 8750 kg/m³. (a) What is the molality of Zn in the solid solution?

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Textbook Question

Commercial concentrated aqueous ammonia is 28% NH₃ by mass and has a density of 0.90 g/mL. What is the molarity of this solution?