Consider this reaction:
$$\ce{CaCO3(s) <=> CaO(s) + CO2(g)}$$
for this, $K_c=\left[\ce{CO2(g)}\right]$
For a given temperature, $K_c$ will remain fixed. That means, the amount of $\ce{CO2}$ released will be same, irrespective of amount of $\ce{CaCO3}$ taken.
But, that means, at the same temperature, irrespective of whether we start with 1 g of $\ce{CaCO3}$, or 10 kg of $\ce{CaCO3}$, the amount of $\ce{CO2}$ at equilibrium will be same(!) because, according to the $K_c$ expression, it should be constant.
This is against my intuition, because, it seems that if we start with 10 kg of $\ce{CaCO3}$, we should end up with a much larger amount of $\ce{CO2}$ at equilibrium than if we started with just 1 g of the carbonate.
Am I being mistaken somewhere, or is this is what will actually happen? I am confused.