for following reaction at equilibrium if we increase the reaction temperature the equilibrium will
2SO3(g)<-->2SO2(g)+O2(g)(deltaH degrees=198kJ)
A. not shift
B.the question can not be answered because Keq is not given
C.shift to the right
D. shift to the left
I am going with D.
Do you agree?
If delta H is + (which is what I read in the post), the reaction is endothermic and can be written as
2SO3 + heat ==>2SO2 + O2
Increasing temperature will make the reaction shift so as to use up the heat which means it will shift to the right.
Actually you are 100% correct and i agree with C.
thankyou so much
To answer the question, we need to apply Le Chatelier's principle. According to Le Chatelier's principle, when a change is imposed on a system at equilibrium, the system responds by shifting in a way that minimizes the effect of the change.
In this case, the reaction is exothermic, meaning it releases heat (198 kJ). Therefore, increasing the temperature would be equivalent to adding heat to the system. To minimize the effect of this temperature increase, the reaction will shift in the direction that absorbs heat.
Looking at the reaction, the forward reaction (2SO3 ⇌ 2SO2 + O2) is slightly favored as indicated by a positive delta H value. Increasing the temperature would cause the reaction to shift to the left in an attempt to consume the added heat. Therefore, the equilibrium will shift to the left, meaning there will be a decrease in the amount of products (SO2 and O2).
So your answer, D. shift to the left, is correct.