Answer:
2.66 x 10^19 CO2 molecules
Explanation:
0.04% = 0.04 / 100 = 0.00040
2.7 L air x (0.00040 L of CO2 is in 1 L air) = 0.00108 L CO2
Use the ideal gas law to find moles of CO2.
PV = nRT
n = PV / RT = (1.00 atm)(0.0012 L) / (0.0821 L atm / K mole)(298 K) = 4.44 x 10^-5 moles CO2
One mole of anything contains 6.02 x 10^23 particles.
4.44 x 10^-5 moles CO2 x (6.02 x 10^23 CO2 molecules / 1 mole CO2) = 2.66 x 10^19 CO2 molecules
Answer:
2.66x10¹⁹ molecules of CO₂
Explanation:
Using ideal gas law (PV = nRT), it is possible to find moles of air collected thus:
PV = nRT
PV / RT = n
1.00atm×2.7L / 0.082atmL/molK×298.15K = n
Temperature in Kelvin (25°C + 273.15 = 298.15K); R is gas constant (0.082atmL/molK)
0.110moles of air you collected. From here, 0.04% is CO₂. Thus, moles of CO₂ are:
0.110moles × (0.04 / 100) = 4.42x10⁻⁵ moles of CO₂. 1 mole contains 6.022x10²³ molecules. Molecules of CO₂ are:
4.42x10⁻⁵ moles of CO₂ × (6.022x10²³ molecules / 1mol) =
2.66x10¹⁹ molecules of CO₂
