I solved this exercise but I doubt something is wrong...
There is no result at the end of it.
"A volume of 4.60 lt SPT of a mixture composed of NO
2 and Cl
2 react with the following reaction:
NO
2 + Cl
2 NO
2Cl
We know that NO
2 is the limiting reagent. The final volume of all the gas is 4.14 lt SPT. Please calculate the starting composition of the mixture".
First of all, I balanced the reaction: 2NO
2 + Cl
2 2NO
2Cl
Than I wrote: V(mixture) = V(NO
2) + V(Cl
2)
V(final) = final V(NO
2) + final V(Cl
2) + final V(NO
2Cl) (at the end)
So I called the final V(NO
2) = x - 2 (2 lt is the volume it should lose after the reaction because of the coefficients) and then I called the final V(Cl
2) = y - 1 (2 lt is the volume it should lose after the reaction because of the coefficients).
So now I have a linear system with two equations:
x + y = 4.60
and
x - 2 + y - 1 + x = 4.14
I solved it and I found that V(NO
2)= 2.54 lt and V(Cl
2)= 2.06 lt so the composition of the starting mixture is:
55.2% of NO
2 and 44,8 % of Cl
2.
I'm really not sure of what I did... especially because of the fact that I didn't use the SPT information about the volumes.
Sorry for my english which is not perfect
Thanks!!!