Carbon dioxide makes up approximately 0.04% of earth's atmosphere. if you collect a 2.7 l sample from the atmosphere at sea level (1.00 atm) on a warm day (25 ∘c), how many co2 molecules are in your sample?

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

the answer is the first option

explanation:

just googled it m8. not that hard

lol

increased stability in the completion of fluorine's outer shell.