hey can any1 help me out?
At 900degrees C, Kp = 1.04 for the reaction
CaCO3 (s) --> CaO(s) + CO2(g)
At a low temperature, dryi ice (solid CO2), calcium oxide and calcium carbonate are introduced into a 50L reaction chamber. The temperature is raised to 900dgrees C, resulting in the dry ice converting to gaseous CO2. For the following mixtures, will the initial amount of calcium oxide increase, decrease or remain the same as the system moves toward equilibrium at 900degrees C?
a) 655g CaCO3, 95.0g CaO, P(CO2) = 2.55atm
b) 780g CaCO3, 1.00g CaO, P(CO2) = 1.04atm
I can do the rest (part c and d) if i know how to do a) or b) so can any1 tell me how i'm meant to approach this question? i really don't know how to start it. for one thing, i realise that only gases would be participating in calculating the pressure equilibrium.
they say the answer is "decreases".