Hello guys!
I'm posting again this problem with a better formatting and I'll show my attempts now. I didn't show my attempts because I was too lazy , but because I thought it was not necessary, and for this I'm really sorry!
The problem is the following
200 g of an organic compound with formula CaC2O4, 100 g of O2 and 50g of N2 are introduced inside a reactor with a constant volume of 100 L kept at 950 °C. The volume of the solid substances can be neglected, being smaller than the reactor volume. The following two reactions take place consecutively:
CaC2O4(s)-->CaO(s)+CO2(g)+CO(g)
2CO(g) +O2(g)-->2CO2(g)
Calculate the final pressure within the vessel.
Ok. So...what I thought was that to calculate the final pressure I have to calculate all partial pressure and then sum them up. So first I need to calculate the number of moles of each compound.
Firstly I calculate the ones I know the mass of, by dividing it by the molar mass. Once I find the number of moles of:
CaC2O4(s)
O2 and N2
I calculate the number of moles of the other compounds multiplying the values I found for CaC2O4(s) and for O2 by each stoichyometric coefficient.
For example number of moles of (2CO2(g)) is equal to: number of moles of (O2) times 2
actually I'm not sure about this.
Anyway, after I found all the number of moles I use the formula: PV=nRT --> P=(nRT)/V
where n is the sum of all number of moles.
Thank you in advance and have a good day!