The equilibrium constant at 1127^∘ C for the following endothermic reaction is 571 : 2 H2 S(g) ⇌

step 1 For this question, we're given an equation, and we know that this is an endothermic reaction, an

The equilibrium constant at 1127^∘ C for the following...

The equilibrium constant at $1127^{\circ} \mathrm{C}$ for the following endothermic reaction is 571 : $$2 \mathrm{H}_{2} \mathrm{S}(g) \rightleftharpoons 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g)$$ If the mixture is at equilibrium, what happens to $K$ if we: (a) Add some $\mathrm{H}_{2} \mathrm{S} ?$ (b) Add some $\mathrm{H}_{2} ?$ (c) Lower the temperature to $1000^{\circ} \mathrm{C} ?$

The equilibrium constant at $1127^{\circ} \mathrm{C}$ for the following endothermic reaction is 571 :
$$2 \mathrm{H}_{2} \mathrm{S}(g) \rightleftharpoons 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g)$$ If the mixture is at equilibrium, what happens to $K$ if we:
(a) Add some $\mathrm{H}_{2} \mathrm{S} ?$
(b) Add some $\mathrm{H}_{2} ?$
(c) Lower the temperature to $1000^{\circ} \mathrm{C} ?$

Key Concepts

Temperature Dependence of the Equilibrium Constant

The equilibrium constant is sensitive to temperature changes because the equilibrium position of a reaction depends on the balance of enthalpy and entropy. For an endothermic reaction, a decrease in temperature results in a smaller value of K since the reaction shifts toward the reactants, whereas an increase in temperature would favor the formation of products, increasing K. Temperature is the only factor among those discussed that can change the value of the equilibrium constant.

Effect of Concentration Changes on Equilibrium

Altering the concentrations of reactants or products will shift the position of the equilibrium in order to partially alleviate the change, but it does not change the value of the equilibrium constant (K). When additional reactant or product is added, the reaction will shift toward the opposite side to re-establish equilibrium, without altering K.

Chemical Equilibrium Constant

The equilibrium constant (K) quantifies the ratio of the concentrations (or partial pressures for gases) of products to reactants at equilibrium. It is a fixed value for a given reaction at a specific temperature and does not change when the concentrations of reactants or products are altered, as long as the temperature remains constant.

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium experiences a change in concentration, pressure, or temperature, the system will adjust its equilibrium position to counteract the imposed change. This principle helps predict the direction of the shift in the reaction when disturbances occur, though the equilibrium constant itself remains unchanged by concentration or pressure changes.

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