Question

Consider the following equilibrium system:

C(s) + H2O(g) <-> СО(g) + H2(g)
Keq= 0.80
In an experiment, a student places 0.10 mol of C, 0.15 mol of H,0,0.25 mol of CO,
and 0.20 mol of H, into a 1.0 L flask. The student predicts that the [CO] will decrease as
equilibrium becomes established.
Would you agree or disagree with the student?
a) Agree
b) Disagree

Answer 1

I disagree with the student's prediction that the concentration of CO will decrease as equilibrium is established.

Step-by-step explanation:

In the given equilibrium system, the student predicts that the concentration of CO will decrease as equilibrium becomes established. I would disagree with the student. According to Le Chatelier's principle, when there is an increase in the concentration of one of the reactants, the equilibrium will shift towards the products to counteract the change. In this case, the student is adding more CO and H2, which are the products. This will cause the equilibrium to shift towards the reactants, resulting in an increase in the concentration of CO.