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: H2(g) + F2(g) 2HF(g) removing H2 will have no effect on the amount of F2 present once equilibrium is reestablished.

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 doubled.

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

For the following reaction at equilibrium: CaCO3(s) CaO(s) + CO2(g) adding more CaCO3 will shift the equilibrium to the right.

For the following reaction at equilibrium: CaCO3(s) CaO(s) + CO2(g) increasing the total pressure by adding Ar(g) will have no effect on the equilibrium position

Explanation / Answer

1)
For the following reaction at equilibrium: H2(g) + F2(g) 2HF(g) removing H2 will have no effect on the amount of F2 present once equilibrium is reestablished.
Removing H2 will shift the reactant to reactant side because H2 is a reactant
Answer: False
2)
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 doubled.
Increasing volume will decrease pressure. So, equilibrium will move to side where there are more gases to increase the pressure. Here more gases are in reactant side, so equilibrium will shift to left
Answer: False
3)
Increasing the temperature of an exothermic reaction shifts the equilibrium position to the right.
Increasing temperature will favour endothermic reaction. Here backward reaction is endothermic. So, equilibrium will be shifted to left
Answer: False
4)
For the following reaction at equilibrium: CaCO3(s) CaO(s) + CO2(g) adding more CaCO3 will shift the equilibrium to the right.
Adding solid do not effect Equilibrium
Answer: False

5)
For the following reaction at equilibrium: CaCO3(s) CaO(s) + CO2(g) increasing the total pressure by adding Ar(g) will have no effect on the equilibrium position
Increasing pressure will will make equilibrium move to side where there are less gases to decrease the pressure. Here less gases are in reactant side, so equilibrium will shift to left
Answer: False

All are false

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