One mole of an ideal gas at 1.00 atm and 0.00 $\degree$C occupies 22.4 L.How many molecules of an ideal gas are in one cm³ under these conditions? A)28.9 B)22 400 C)2.69 x 10¹⁹ D)6.02 x 10²³

Question

Quizplus · Accepted Answer

First, we need to use the ideal gas law to find the number of moles of gas in the 22.4 L container:
PV = nRT
(1.00 atm)(22.4 L) = n(0.0821 L∙atm/mol∙K)(273 K)
n = 1 mol

Now we need to use Avogadro's number to convert from moles to molecules:
1 mol = 6.02 x 10^23 molecules

Finally, we need to use dimensional analysis to convert from L to cm^3:
1 L = 1000 cm^3
22.4 L = 22,400 cm^3

So the total number of molecules in 1 cm^3 under these conditions is:
(6.02 x 10^23 molecules/mol) / (22,400 cm^3) = 2.69 x 10^19 molecules/cm^3

Therefore, the correct answer is C.

One Mole of an Ideal Gas at 1 °\degree° C Occupies 22

One Mole of an Ideal Gas at 1 $\degree$ C Occupies 22