At a low temperature dry ice (solid CO2), calcium oxide, and calcium carbonate are introduced into a 50.0-L reaction chamber. The temperature is raised to 900.! C. For the following mixtures, will the initial amount of calcium oxide increase, decrease, or remain the same as the system moves toward equilibrium

the initial amount of calcium oxide will decrease as the system moves toward equilibrium

Explanation:

The question should have this variable:

a) 655g CaCO3, 95.0g CaO, P (CO2) = 2.55atm

The reaction formula of dry ice, calcium oxide and calcium carbonate should be:

CaCO3 (s) - -> CaO (s) + CO2 (g)

With Kp = 1.04 at 900 degrees C

in this tank, only CO2 (g) is in gaseous form. The amount of gas will determine the pressure of the tank. When the tank heated, its temperature rise and will also rise the pressure. When pressure higher than Kp, the equilibrium will shift toward side with less gas.

There is only one gas in the reaction, so Kp = P (CO2)

Since P (CO2) is 2.55 atm and its higher than Kp (1.04), the equilibrium will shift to the left. Since the reaction direction to the left, the amount of calcium carbonate will increase while carbon dioxide and calcium oxide will decrease.