Question

Given the eqilibrium equation SO₂Cl_2(g) --> SO_2(g)+Cl_2(g) , with a heat of reaction of +67 kj, the concentration of sulfur dioxide at equilibrium can be increased by:

-Increasing the temperature

-removing the SO₂Cl_2(g)

-decreasing the volume of the reaction vessel

If you could explain why the option is correct it would be much appreciated :)

Answer 1

1)
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 and SO2 will increase

2)
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 and SO2 will decrease

3)
We are decreasing volume here
In other words we are trying to increase pressure
so, according to Le Chatelier's principle,
Reaction will try to decrease the pressure
Hence it will move in a direction which have lesser gaseous molecules
Here reactant has less gaseous molecule
So equilibrium will move to left
Answer: Equilibrium moves to reactant side and SO2 will decrease

Answer: option 1