Consider the following reaction that has reached equilibrium:
H2 (g) + F2 (g) 2HF (g) ∆H = 541 kJ
What will happen to the concentration of HF if the temperature is lowered?
What will happen to the concentration of H2 if the temperature is raised
Can someone please help me with this chemistry question?
2017-08-11 4:29 pm
回答 (1)
2017-08-11 4:37 pm
H₂(g) + F₂(g) ⇌ 2HF(g) …. ∆H = 541 kJ
A positive ΔH corresponds to an endothermic forward reaction and an exothermic backward reaction.
According to Le Chatelier's principle, low temperature favors the exothermic reaction, i.e. the backward reaction. Therefore, when temperature is lowered, the equilibrium position will shift to the left. This leads to the decrease in the concentration of HF.
According to Le Chatelier's principle, high temperature favors the endothermic reaction, i.e. the forward reaction. Therefore, when temperature is raised, the equilibrium position will shift to the right. This leads to the decrease in the concentration of H₂.
A positive ΔH corresponds to an endothermic forward reaction and an exothermic backward reaction.
According to Le Chatelier's principle, low temperature favors the exothermic reaction, i.e. the backward reaction. Therefore, when temperature is lowered, the equilibrium position will shift to the left. This leads to the decrease in the concentration of HF.
According to Le Chatelier's principle, high temperature favors the endothermic reaction, i.e. the forward reaction. Therefore, when temperature is raised, the equilibrium position will shift to the right. This leads to the decrease in the concentration of H₂.
收錄日期: 2021-05-01 13:46:15
原文連結 [永久失效]:
https://hk.answers.yahoo.com/question/index?qid=20170811082927AAmxLCn