Assume that the air in this problem is an ideal gas with a composition that is 78.0% N2 and 22.0% O2. (a) How many moles of air are in a volume of one cubic meter at room temperature (293.15 K) at a pressure of one atmosphere

41.6 moles

Explanation:

We apply the Ideal Gases Law to solve this:

P . V = n . R . T

Volume is 1m³ but we need to convert to dm³ (L), because the units of R

1m³ . 1000 dm³/1m³ = 1000 dm³ → 1000L

Now we replace → 1 atm . 1000 L =  n . 0.082L.atm/mol.K . 293.15K

(1 atm . 1000 L) / (0.082L.atm/mol.K . 293.15K) = n → 41.6 moles

8 carbon atoms forming single bonds with 18 hydrogen atoms; a triple bond exists between the third and fourth carbon atom from the right

explanation:

a compound is a molecule made of atoms from different elements.

a. by the combination of an unlimited number of elements