Calculate the volume of chlorine that is required to convert 1 kg of iron in ferric 3 chloride at standard conditions?

1 Answer
anor277
Apr 28, 2016

Approx. #600*L# at #"STP"#.

Explanation:

#Fe(s) + 3/2Cl_2(g) rarr FeCl_3(s)#

Moles of iron #=# #(1000*cancelg)/(55.85*cancelg*mol^-1)# #=# #17.91*mol#.

Given the rxn stoichiometry, we need at a bare minimum, #3/2# this molar quantity of chlorine gas, i.e. #26.9# #mol# #Cl_2# gas.

Now I know that under standard condtions, #1# #mol# of ideal gas has a volume of #22.4*L#. (This would be given as supplementary material in any examination!).

Thus #26.9*cancel(mol)xx22.4*L*cancel(mol^-1)# #=# #??*L#

Related questions
See all questions in Equation Stoichiometry
Impact of this question
2256 views around the world
You can reuse this answer
Creative Commons License