[mudkip26]

Decide which of the following statements are True and which are False about equilibrium systems:
My answers will be in blue!

 For the following reaction: CaCO3(s) ⇌ CaO(s) + CO2(g) the [CaCO3] appears in the denominator of the equilibrium expression. True

 The value of K at constant temperature depends on the amounts of reactants and products that are mixed together initially. False

 For a reaction with K >> 1, the rate of the forward reaction is less than the rate of the reverse reaction at equilibrium. False

 A large value of K means the equilibrium position lies far to the right. True

 For the following reaction: H2(g) + F2(g) ⇌ 2HF(g) the values of K and Kp are not the same. True


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For the following exothermic reaction at equilibrium:
H2O (g) + CO (g) CO2(g) + H2(g)

Decide if each of the following changes will increase the value of K (T = temperature).


 Add CO (constant T) No

 Add Ne(g) (constant T) No

 Remove CO (constant T) No

 Decrease the volume (constant T) No

 Decrease the T Yes

 Add a catalyst (constant T) No

 Increase the T Yes

NOTE: K IS NOT THE TEMPERATURE! K IS THE EQUILIBRIUM CONSTANT!

[Big-Daddy]

Decide which of the following statements are True and which are False about equilibrium systems:
My answers will be in blue!

 For the following reaction: CaCO3(s) ⇌ CaO(s) + CO2(g) the [CaCO3] appears in the denominator of the equilibrium expression. True

 The value of K at constant temperature depends on the amounts of reactants and products that are mixed together initially. False

 For a reaction with K >> 1, the rate of the forward reaction is less than the rate of the reverse reaction at equilibrium. False

 A large value of K means the equilibrium position lies far to the right. True

 For the following reaction: H2(g) + F2(g) ⇌ 2HF(g) the values of K and Kp are not the same. True


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For the following exothermic reaction at equilibrium:
H2O (g) + CO (g) CO2(g) + H2(g)

Decide if each of the following changes will increase the value of K (T = temperature).


 Add CO (constant T) No

 Add Ne(g) (constant T) No

 Remove CO (constant T) No

 Decrease the volume (constant T) No

 Decrease the T Yes

 Add a catalyst (constant T) No

 Increase the T Yes

NOTE: K IS NOT THE TEMPERATURE! K IS THE EQUILIBRIUM CONSTANT!

I agree with all answers but not too sure about the last one - my guess is that it's probably false but I'm probably making an amateurish mistake here. After all is it not just the reverse of decreasing the temperature slightly further up the page? I'm not sure, I am probably missing something obvious here, I'd like to be corrected by someone more knowledgeable ...

[Borek]

For the following reaction: CaCO3(s) ⇌ CaO(s) + CO2(g) the [CaCO3] appears in the denominator of the equilibrium expression. True

It can be a trick question. There is no such thing as a concentration of CaCO₃. Activity of a solid is always 1.

For a reaction with K >> 1, the rate of the forward reaction is less than the rate of the reverse reaction at equilibrium. False

If the question asks to compare rates at equilibrium, they are not different.