I need to describe and explain the shift in the following reaction using the le chatelier principle (which I understand, I'm just confused with this particular example).
4HCL(g)+O2(g)--><--2H2O(g)+2CL2(g)+113kj The temperature is decreased.
Equilibrium question?
2017-11-09 3:46 pm
回答 (1)
2017-11-09 3:55 pm
4HCl(g) + O₂(g) ⇌ 2H₂O(g) + 2Cl₂(g) + 113kJ
The forward reaction is exothermic, while the backward reaction is endothermic.
According to Le Chatelier's principle, when temperature decreases, it favors the exothermic reaction (forward reaction) to release heat in order to encounter the temperature decrease. Therefore, the equilibrium position shifts to the right.
The forward reaction is exothermic, while the backward reaction is endothermic.
According to Le Chatelier's principle, when temperature decreases, it favors the exothermic reaction (forward reaction) to release heat in order to encounter the temperature decrease. Therefore, the equilibrium position shifts to the right.
收錄日期: 2021-04-24 00:52:40
原文連結 [永久失效]:
https://hk.answers.yahoo.com/question/index?qid=20171109074611AAuSN6q