The reaction below is at equilibrium at a temperature T. There are four possible changes listed. Select all the changes that will shift the equilibrium so as to produce more products
MgO(s) + SO3(g) + 95 kJ <======> MgSO4(s)
I – Increase the temperature
II – Increase the volume
III – Add more MgO
IV – Remove SO3
I)
Forward reaction is endothermic in nature
we are increasing temperature or adding heat here
so, according to Le Chatelier's principle,
equilibrium will move in direction which absorbs heat
hence, forward reaction will be favoured
Answer: Equilibrium moves to product side
II)
We are increasing volume here
In other words we are trying to decrease pressure
so, according to Le Chatelier's principle,
Reaction will try to increase the pressure
Hence it will move in a direction which have more gaseous molecules
Here reactant has more gaseous molecule
So equilibrium will move to left
Answer: Equilibrium moves to reactant side
III)
Adding solid or liquid doesn't affect equilibrium
Answer: No effect on equilibrium
IV)
we are removing a reactant
According to Le Chatelier's Principle,
Removing reactant will shift reaction towards reactant side
Answer: Equilibrium moves to reactant side
Answer: I
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