How many molecules are there in 15.7 liters of chlorine gas at STP?

1 Answer
anor277
Apr 12, 2016

#(15.7*L)/(22.414*L*mol^-1)# #xx# #N_A#

Explanation:

We idealize the behaviour of this gas. And it is a fact that #STP#, 1 mole of an ideal gas has a volume of #22.414*L#.

So we take the quotient, #(15.7*L)/(22.414*L*mol^-1)# to get a molar quantity, and multiply this amount by Avogadro's number to get the number of molecules.

#(15.7*cancelL)/(22.414*cancelL*cancel(mol^-1))# #xx# #6.022xx10^23*cancel(mol^-1)# #=# #??#

How many individual chlorine atoms are there in this quantity?

Related questions
See all questions in Molar Volume of a Gas
Impact of this question
8891 views around the world
You can reuse this answer
Creative Commons License