posted by Hannah .
For each of the following equilibria, use Le Chatelier's principle to predict the direction of reaction when the volume is increased.
(a) C(s) + H2O(g) CO(g) + H2(g)
(b) 2 H2(g) + O2(g) 2 H2O(g)
(c) 2 Fe(s) + 3 H2O(g) Fe2O3(s) + 3 H2(g)
a i put no change because there are the same number of moles of on both-it was wrong
b i put shift towards prodcuts. because it has less moles but it was wrong
and c i put shift towards products but it was wrong. please help!
It's mols of GAS you should be counting. In a you have 1 mol on the left and 2 on the right. C solid doesn't count.
c has 3 on left and 3 on right.
for a would be toward reactants?
I don't think so. When pressure is increased the reaction shifts to the side with the fewer mols. For a volume increase, pressure is decreased so rxn shifts to side with more mols; therefore, it shifts to the right.