Which of the following are true statements about equilibrium systems? For the fo

Question

Which of the following are true statements about equilibrium systems? For the following reaction at equilibrium:

1. CaCO3(s) CaO(s) + CO2(g) adding more CaCO3 will shift the equilibrium to the left.

2. Increasing the temperature of an exothermic reaction shifts the equilibrium position to the right.

3. For the following reaction at equilibrium: 2 H2(g) + O2(g) 2 H2O(g) the equilibrium will shift to the right if the volume is halved.

4. For the following reaction at equilibrium: H2(g) + F2(g) 2HF(g) removing H2 will decrease the amount of F2 present once equilibrium is reestablished.

5. For the following reaction at equilibrium: CaCO3(s) CaO(s) + CO2(g) increasing the total pressure by adding Ar(g) will shift the equilibrium to the left.

Explanation / Answer

1)we are adding a reactant

According to LeChattelier's Principle,

Adding reactant will shift reaction towards product side

Equilibrium moves to product side

Answer: False

2)Forward reaction is exothermic in nature

we are increasing temperature or adding heat here

so, according to Le Chatellier's principle,

equilibrium will move in direction which absorbs heat

hence, backward reaction will be favoured

Equilibrium moves to reactant side

Answer: false

3)We are decreasing volume here

In other words we are trying to increase pressure

so, according to Le Chatellier's principle,

Reaction will try to decrease the pressure

Hence it will move in a direction which have lesser gaseous molecules

Here product has less gaseous molecule

So equilibrium will move to right

Equilibrium moves to product side

Answer: true

4)we are removing a reactant

According to LeChattelier's Principle,

Removing reactant will shift reaction towards reactant side

Equilibrium moves to reactant side

Answer: false

5)We are increasing pressure here

so, according to Le Chatellier'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

Equilibrium moves to reactant side

Answer: true

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