Answer to Question #300393 in General Chemistry for Barbosa

Question

Steam reacts reversibly with iron at red-heat in the following way.

3Fe(s)+4H 2 O(g) rightleftharpoons Fe 3 O 4 (s)+4H 2 (g)

Describe and explain what happens when the conditions of the reaction are varied as follows:

(a) Increasing the partial pressure of the steam.

(b) Adding more of the iron (I] ) diiron * (IV) oxide, F*e_{3} * O_{4}

(c) Removing the hydrogen gas formed.

Answer 1

3Fe + 4H2O <--> Fe3O4 + 4H2 +Q

substitution, reversible, redox, exothermic, heterogeneous

a)An increase in pressure shifts the equilibrium towards a decrease in the total number of gas molecules, and a decrease in pressure - towards an increase in the number of molecules.

increase in pressure in a reaction

will lead to a shift in equilibrium towards a direct reaction, since as a result of its occurrence, the total number of gas molecules will decrease.

If the reaction proceeds without changing the number of moles of gaseous substances, then pressure changes do not affect the equilibrium shift.

b)the introduction of reaction products into the system leads to a shift in the equilibrium towards the reverse reaction

c)A decrease in concentration contribute to a shift in equilibrium towards its formation, i.e., towards a direct reaction.