Answer:
According to Le Chatelier's principle, a change in conditions of a system at equilibrium will cause the system to shift in a way that opposes the change. However, some changes do not affect the position of equilibrium.
In the given equilibrium system:
H₂(g) + F₂(g) ⇌ 2HF(g) ΔH < 0
where ΔH is the enthalpy change for the reaction, which is negative, indicating that the reaction is exothermic.
Since heat is included in the equation, a change in temperature would affect the position of the equilibrium. Specifically, an increase in temperature would favor the endothermic reaction (i.e., the reactants side), while a decrease in temperature would favor the exothermic reaction (i.e., the products side).
On the other hand, changes in pressure and concentration will shift the equilibrium position. For example, an increase in pressure would shift the equilibrium to the side with fewer moles of gas (in this case, the products side), while an increase in concentration of one of the reactants or products would shift the equilibrium away from that species.
Therefore, a change in heat that does not affect the temperature of the system will not shift the equilibrium position. For example, adding a catalyst or changing the volume of the container (as long as it does not change the pressure) will not affect the position of equilibrium.
Step-by-step explanation:
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