Question

For each of the following equilibria, use Le Chatelier's principle to predict the direction of reaction when the volume is increased. Drag the appropriate chemical equations to their respective bins.

chemical equations: 2H2(g)+ O2 (g) ⇌ 2H2O (g), C (s) + H2O (g) ⇌ CO (g) + H2 (g), 2Fe (s) + 3H2O (g) ⇌ Fe2O3 (s) + 3H2 (g)

bins: Reaction will go toward products, Reaction will go toward reagents, Reaction will remain at equilibrium

Answer 1

Answer

Reaction go toward products: C(s) + H2O(g) <-------> CO(g) + H2(g)

Reacion will go toward reagents : 2H2(g) + O2(g) <------> 2H2O(g)

Reaction will remain at equilibrium : 2Fe(s) +3H2O(g) <-------> Fe2O3(s) + 3H2(g)

Explanation

According to Lechatler principle, If a change such as change in concentration , change in pressure , change in volume or change in temperature is applied to an chemical equilibrium , the equilibrium adjust itself as the counter act to the applied change.

As volume increased pressure will decrease. As the counter act to decrease in pressure, the equilibrium shift to the higher gaseous molar side.

2H2(g) + O2(g) <-------> 2H2O(g) : higher gaseous molar side is reactant side, so , equilibrium shift to reagent side

C(s) + H2O(g) <------> CO(g) + H2(g) : higher gaseous molar side is product side , so, equilibrium shift to product side.

2Fe(s) + 3H2O(g) <-------> Fe2O3(s) + 3H2(g) : both sides are equal gaseous moles , so, no change in the equilibrium.