I would look at it this way.
A is missing only H2O so it can move to the left to reach equilibrium.
B is missing the right side so it can move to the right.
C is missing the left side so it can move to the left.
D is missing something on the left AND something on the right. That means CO must decrease and H2 must decrease. If it moves to the left to decrease H2 what happens to the CO2. It increases but it must decrease. Right? If it moves to the right to decrease CO2 what happens to the H2. It increases but it must decrease. So this one can't work.
Consider the reaction:
CO(g) + H2O (g) <---> CO2(g)+H2(g)
which of the following initial composition will NOT achieve equlibrium?
a) 0.25 mol H2, 0.35 mol CO2, and 0.25 mol CO
b) 0.25 mol CO, 0.75 mol H2O
c) 1.0 mol of CO2 and 0.50 mol H2
d) 0.85 mol CO and 0.25 mol H2
how do i do this? i can't make an ICE table because no volume is given. which means i can't find Keq or Q . So how else am i supposed to reason this?
2 answers
yes that makes sense, thank you!!