For the following endothermic reaction system at equilibrium: 2SO3(g) <---> 2SO2(g) + O2(g) Choose the changes...

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Question

For the following endothermic reaction system at equilibrium: 2SO3(g) <---> 2SO2(g) + O2(g) Choose the changes...

For the following endothermic reaction system at equilibrium:

2SO₃(g) <---> 2SO₂(g) + O₂(g)

Choose the changes that will shift the equilibrium position to the right.

(Select all that apply.)

Add Ne(g)

Add SO₂(g)

Remove SO₃(g)

Decrease temperature

Add a catalyst

Increase temperature

Decrease volume

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Answer 1

Answer #1

A system is said to be in equilibrium when the change in Gibb's free energy is zero.

According to Le Chatlier's Principle, any change is made to a system in equilibrium, it will rearrange so as to attain the equilibrium back.

If we increase the concentration then it shifts to the side of lower concentration.

If we increase the temperature the system shifts to the side of endothermic reaction side. If we decrease the temprature it shifts to the exothermic side.

If we increase the pressure the system shifts from the highest number of moles side to the lowest number of moles side.

If we introduce a inert gas there will be no effect on equilibrium. The catalyst also doesn't have effect on equilibrium.

Here the question is when the equilibrium will shift to the right.

It will happen if we increase the concentration of SO3, decrease the pressure, increase the temperature, increase the volume.

The answer is

Increase temperature.

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Answer 2

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For the following endothermic reaction system at equilibrium: 2SO3(g) <---> 2SO2(g) + O2(g) Choose the changes...

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Add Answer to: For the following endothermic reaction system at equilibrium: 2SO3(g) <---> 2SO2(g) + O2(g) Choose the changes...

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For the following endothermic reaction system at equilibrium: 2SO3(g) <---> 2SO2(g) + O2(g) Choose the changes...