Air consists of molecules of several types, with an average molar mass of 28.95 g. An adult who inhales 0.6 L of air at sea level takes in about how many molecules? (The density of air is 1.229 kg/m^3, and the molar mass of air is 28.95 g/mol.)
0.6 L = 6*10^-4 m^3
The mass of that volume is
6*10^-4*1.229 kg , which is
0.737 grams.
Divide that by 28.95 g/mol for the number of moles. Then multiply that by Avogadro's number for the number of molecules.
tyvm :)
To calculate the number of molecules in the given volume of air, we can follow these steps:
Step 1: Convert the given volume from liters (L) to cubic meters (m³).
1 liter (L) = 0.001 cubic meters (m³)
0.6 L = 0.6 x 0.001 = 0.0006 m³
Step 2: Use the density of air to calculate the mass of the given volume of air.
Density = Mass / Volume
Mass = Density x Volume
The density of air is given as 1.229 kg/m³, and the volume of air is 0.0006 m³.
So, Mass = 1.229 kg/m³ x 0.0006 m³ = 0.0007374 kg
Step 3: Calculate the number of moles of air using the molar mass of air.
Molar mass of air = 28.95 g/mol
To convert the mass from kg to grams:
0.0007374 kg = 0.0007374 kg x 1000 g/kg = 0.7374 g
Number of moles = Mass / Molar mass
Number of moles = 0.7374 g / 28.95 g/mol ≈ 0.0255 mol
Step 4: Calculate the number of molecules using Avogadro's number.
Avogadro's number (Nₐ) = 6.022 x 10²³ molecules/mol
Number of molecules = Number of moles x Avogadro's number
Number of molecules = 0.0255 mol x (6.022 x 10²³ molecules/mol)
Number of molecules ≈ 1.535 x 10²²
Therefore, an adult who inhales 0.6 L of air at sea level takes in approximately 1.535 x 10²² molecules.