Step-by-step explanation:
To determine the direction the equilibriums will shift and how the temperature change will affect the value of K for each given reaction, we need to consider Le Chatelier's principle and the effect of temperature changes on equilibrium constants.
Le Chatelier's principle states that when a system at equilibrium is subjected to a change in temperature, pressure, or concentration of reactants or products, the system will respond by shifting the equilibrium to counteract the change.
a. N2(g) + 3 H2(g) ⇌ 2 NH3(g) + energy
In this exothermic reaction, energy is a product, and increasing the temperature will shift the equilibrium to the left, favoring the reactants. This is because the system will try to counteract the increase in temperature by consuming some of the added heat (energy) through the reverse reaction. As a result, the concentration of NH3 will decrease, and the concentration of N2 and H2 will increase.
For this reaction, the value of K will decrease at higher temperatures due to the shift in equilibrium favoring the reactants.
b. H₂O(l) ⇌ H₂O(g)
This is a phase change equilibrium between liquid water and water vapor. The forward reaction is the evaporation of liquid water to form water vapor (gas). Increasing the temperature will shift the equilibrium to the right, favoring the formation of more water vapor. The concentration of water vapor will increase while the concentration of liquid water will decrease.
For this reaction, the value of K (the equilibrium constant) remains unchanged as it is a ratio of concentrations of products and reactants, and the stoichiometric coefficients are both 1.
c. CO(g) + 2 H2(g) ⇌ CH3OH(l) + heat
In this reaction, heat is a reactant, and it is an exothermic reaction. When the system is heated, the equilibrium will shift to the left, favoring the formation of more reactants (CO and H2) and less product (CH3OH). This is to counteract the increase in temperature and consume some of the added heat through the reverse reaction.
For this reaction, the value of K will decrease at higher temperatures due to the shift in equilibrium favoring the reactants.
d. 8 ZnS(g) ⇌ 8 Zn(g) + S8(g)
This reaction involves the decomposition of zinc sulfide (ZnS) into zinc (Zn) and sulfur (S8) gas. This is an endothermic reaction, and increasing the temperature will shift the equilibrium to the right, favoring the formation of more products (Zn and S8 gas). The concentration of Zn and S8 gas will increase.
For this reaction, the value of K will increase at higher temperatures due to the shift in equilibrium favoring the products.
In summary:
a. The equilibrium will shift to the left, and K will decrease.
b. No shift in equilibrium, and K remains unchanged.
c. The equilibrium will shift to the left, and K will decrease.
d. The equilibrium will shift to the right, and K will increase.