Question on Le Chatelier's theory?

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In the discussion about Le Chatelier's principle, a reversible exothermic reaction is analyzed under the influence of a constant heat source that raises the system's temperature by 10 degrees Celsius. The reaction, A + B --> C + D, shifts to the left in response to the added heat, as predicted by Le Chatelier's principle. However, the continuous heating from the heater means that the temperature will not return to the original X degrees Celsius but will stabilize at X + 10 degrees. The consensus is that while the reaction attempts to counteract the temperature increase by favoring the reverse reaction, it cannot overcome the constant heat input. Thus, the final temperature remains X + 10.
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Homework Statement



I have a system which is at X degree celcius. I decide to put in a heater which will heat the system up by 10 degree celsius and will keep supplying this much heat. The reaction taking place is:

A + B --> C + D (it's a reversible reaction)
(enthalpy change is negative-> Exothermic)

I know the reaction will move to the left, but will the temperature of the system be X? Or X + 10?

I mean the reaction is moving backwards in order to eliminate these disturbance in temperature, will it succeed in lowering the temperature to X? Or will it just keep trying by continuously favouring the backward reaction?



The Attempt at a Solution



I formulated this question myself because of my misunderstanding.
 
Last edited:
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I think the answer is X + 10. The reaction will move to the left, but the temperature of the system will be X + 10 because the heater is continuously supplying heat.
 
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