Consider four identical 1.0-L flasks containing the following gases each at 0°C and 1 atm pressure. Which sample has the most molecules? Multiple Choice SO2 H2 O2 same for all gases NH3

The number of molecules is the same for all gases

Explanation:

Using general ideal gas law:

PV = nRT

PV/RT = n

It is possible to find moles of a gas knowing its pressure (1atm), volume (1.0L) and absolute temperature (0+273.15 = 273.15K). R = 0.082atmL/molK

1atm*1.0L/0.082atmL/molK*273.15K = n

0.0446 moles = n

These 0.0446moles are the moles of an ideal gas under these conditions. In an ideal gas its nature is indifferent, that means if you have these four gas under these identical conditions, the number of molecules is the same for all gases.

the correct answer is option d

explanation:

i was wrong its d because they dont use cm when calculating square roots