Sorry but this really confuses me. Wouldn't adding powdered FeO increase the concentration which would then in turn force the reaction to the products side?
Can someone also explain adding FeO would increase the reaction rate as well?
The question, as presented by the OP, states:
"Consider the following reaction:
FeO(s) + CO(g) (double arrow) Fe(s) + CO2(g) ΔH = –283kJ
Which of the following changes to equilibrium conditions
would favour the formation of iron?
A
the addition of more finely powdered FeO
B an increase in temperature
C a decrease in pressure
D the removal of carbon dioxide "
now i take 'the addition of more finely podered FeO' to mean 'instead of adding FeO in blobs, illa dd FeO as a powder'. I can see how u might take it as the addition of MORE FeO, which (you are right) would be correct. However, like i said in my previous post, i believe they added a) to test wheher you know about reaction rates compared to equilibrium.
You would agree, though, D is definitely correct? they can get away with this Q in a HSC because u have to choose the MOST CORRECT answer, and to me D is most definitely correct, while A is incorrect if you take it as i took it (more finely powdered FeO instead of a blob of FeO, not as in add more FeO and let it be finely podered).
Sometimes you have to analyse the Q and teh options - why would they mention 'more finely podered FeO'? Then it clicks - reaction rate increases. But by now you would have eliminated B and C as correct options, so youa re left with A and D. And you have doubt over A because it could mean what i took it to mean, so your safest option is D, which is definitely correct.
PS. Nail the MC in exams, trust me it helps =)
