how will the following system at equilibrium shift in each of thefollowing cases
ID: 683183 • Letter: H
Question
how will the following system at equilibrium shift in each of thefollowing cases?2SO3(g) <---------> 2SO2(g) + O2(g) Ho = 197 kj
a) SO2(g) is added
b) the pressure is decreased by increasing the volume of thecontainer
c) the pressure is increased by adding Ne(g)
d) thetemperature is decreased
e) O2(g) is removed
what a i wrote was:
a) equilibrium shifts to the left because of the increasedconc'n
b) equilibrium shifts to the right to increase the pressure
c) no effect on equilibrium since its a noble gas and is inert
d) equilibrium shifts to the left since its an endothermicreaction, the temp needs to increase
e) equilibrium shifts to the right to replace the oxygen removedfrom the system
are my answers correct?
Explanation / Answer
Yes all of your answers are correct, but the reason for part D isslightly different. For exothermic reactions, heat is a product. For endothermicreactions, heat is a reactant. So by removing heat, we are removinga reactant, which would shift the equilibrium left tocompensate.
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