concentration of water vapor = (31/18)*(1/13) = 0.132 M
3 Fe(s) + 4H2O(g)
<-----> Fe3O4(s) + 4H2(g)
initial excess 0.132 M 0 0
change -4x 4x
equilibrium 0.132-4x 4x
Kc = [H2]^4/[H2O]^4
4 = (4X)^4/(0.132-4X)^4
X = 0.0193
At equilibrium,
[H2] = 4X = 4*0.0193 = 0.0772 M
[H2O] = 0.132-4X = 0.132-4*0.0193 = 0.0548 M
Problem 1. T he reaction of iron and water vapor results in an equilibrium 3 Fe(s)...
The reaction of iron and water vapor results in an equilibrium 3 Fe(s) + 4 H2O (g) ⇋ Fe3O4 (s) + 4 H2 (g) Kc = 5.0 at 800.°C. What is the concentration of water present (in M) at equilibrium if the reaction is initiated with 7.5 g of H2 and excess Fe3O4 in a 15.0 liter container?
B. A scientist had mixed both reactants and products together in a reaction vessel. After some time, thinking the reaction had reached equilibrium, she found that there was 16.6 atm gaseous H2 and 40.0 atm gaseous H2O along with 4.55 g Fe and 3.62 g Fe:04. Had the reaction reached equilibrium? If not, in which direction would the reaction have proceeded to reach equilibrium? EXPLAIN 3. For the given reaction Kp = 0.313: 3Fe(s) + 4H2O(g) =Fe304(s) + 4H2(g) A....
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