I exactly don't know how to solve the final part of this exercise.
"PCl
5 is put in a container which is initially empy and of the volume of 10,00 lt. Temperature is 600 °C. When the equilibrium of the reaction is established
PCl
5 PCl
3 + Cl
2the final pressure in the container is 2,70 atm; 10,40 g of Cl
2 are formed. Calculate K
c and the initial mass of PCl
5"
First of all, I find the n(Cl
2) in equilibrium: 10,40/70,90 = 0,146 (these ones are also equal to n(PCl
3) in equilibrium.
Thanks to the ideal gas law I can calculate the total numer of moles in equilibrium: n(total) = (p * V) / (R * T) = 0,377
n(PCl
5) in equilibrium is: 0,377 - 0,146 - 0,146 = 0,085
So: Kc = (0,146 * 0,146)/(0.085) * 1/10 = 0,025
Now I don't know how to find the initial moles of PCl
5....
Should they be equal to the total moles in equilibrium or not?
Thanks for help.