Consider the following equilibrium, for which ? H < 0 2SO2( g )+O2( g )?2SO3( g

Question

Consider the following equilibrium, for which ?H< 0
2SO2(g)+O2(g)?2SO3(g)
How will each of the following changes affect an equilibrium mixture of the three gases?

Part A

O2(g) is added to the system

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Part B

the reaction mixture is heated

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Part C

the volume of the reaction vessel is doubled

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Part D

a catalyst is added to the mixture

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Part E

the total pressure of the system is increased by adding a noble gas

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Part F

SO3(g) is removed from the system

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Consider the following equilibrium, for which ?H< 0
2SO2(g)+O2(g)?2SO3(g)
How will each of the following changes affect an equilibrium mixture of the three gases?

Part A

O2(g) is added to the system

is added to the system shift equilibrium to the right shift equilibrium to the left no affect

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Part B

the reaction mixture is heated

the reaction mixture is heated shift equilibrium to the right shift equilibrium to the left no affect

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Part C

the volume of the reaction vessel is doubled

the volume of the reaction vessel is doubled shift equilibrium to the right shift equilibrium to the left no affect

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Part D

a catalyst is added to the mixture

a catalyst is added to the mixture shift equilibrium to the right shift equilibrium to the left no affect

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Part E

the total pressure of the system is increased by adding a noble gas

the total pressure of the system is increased by adding a noble gas shift equilibrium to the right shift equilibrium to the left no affect

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Part F

SO3(g) is removed from the system

is removed from the system shift equilibrium to the right shift equilibrium to the left no affect

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Explanation / Answer

a)

Adding reactant will shift the reaction in the direction of product as per Le chatelier Principle

So, Equilibrium moves to product side

Answer: shift equilibrium to the right

b)

Increasing Temperature will shift the reaction in a direction which absorbs heat as per Le chatelier Principle

Forward reaction is exothermic in nature

hence, backward reaction will be favoured

So, Equilibrium moves to reactant side

Answer: shift equilibrium to the left

c)

Increasing volume will decrease the pressure which in turn shift the reaction in a direction which have greater gaseous molecules as per Le chatelier Principle

Here reactant has more gaseous molecule

So equilibrium will move to left

So, Equilibrium moves to reactant side

Answer: shift equilibrium to the left

d)

Catalyst doesn't affect equilibrium

So, No effect

e)

Increasing pressure will shift the reaction in a direction which have lesser gaseous molecules as per Le chatelier Principle

Here product has less gaseous molecule

So equilibrium will move to right

So, Equilibrium moves to product side

Answer: shift equilibrium to the right

f)

Removing product will shift the reaction in the direction of product as per Le chatelier Principle

So, Equilibrium moves to product side

Answer: shift equilibrium to the right

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