Equilibria conundrum

[JaidynM]

My chem teacher was trying to explain the role of solids in equilibrium using an equation that I think was;
CaCO3(s) <--> CaO(s) + CO2(g)

As the concentration of solids are discounted as a constant value of 1, the equilibrium constant, K, would thus be equal to [CO2]. We'd previously learnt that only temperature can effect the value of K; however, by changing the pressure in which the reaction takes place (and through this, the volume), [CO2] would also change. As a result, wouldn't the value of K change with it?

[keltingmeith]

Remember your gas laws. If you change pressure, something had to change with it. Remember:

PV=nRT

Now, n and R can't change (semi-obviously), leaving only volume and temperature. Assuming that volume can't change (which is often the case), then temperature will change. Hence why k changes when you change the pressure.

[JaidynM]

So in this instance a change in temperature occurs alongside the change in pressure? So it isn't the change in pressure changing the value of K but instead the change in temperature?