Question

Three identical flasks contain three different gases at standard temperature and pressure. Flask A contains flask B contains O3, and flask C contains N2. Which flask contains the largest number of molecules? A) flask A B) flask B C) flask C D) All contain same number of molecules.

Answer 1

Answer: All the flasks contain same number of molecules.

Explanation:

STP conditions are called as standard temperature and pressure conditions.

At this condition, 1 mole of a gas occupies a volume of 22.4 L

Also,

The temperature at this condition is taken as 273.15 K  and the pressure at this condition is taken as 1 atm.

According to mole concept:

1 mole of a gas occupies $6.022\times 10^{23}$ number of molecules

We are given:

Three different flasks having three different gases at STP

So, all the flasks will have same number of molecules that is $6.022\times 10^{23}$

Hence, all the flasks contain same number of molecules.