# Problem: At 900ºC, Kp = 1.04 for the reaction CaCO3(s) ⇌ CaO(s) + CO2(g)At a low temperature, dry ice (solid CO 2), calcium oxide, and calcium carbonate are introduced into a 50.0-L reaction chamber. The temperature is raised to 900ºC, 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 900ºC? c. 0.14 g CaCO3, 5000 g CaO, PCO2 = 1.04 atm

###### FREE Expert Solution

We are being asked to determine whether the initial amount of calcium oxide increase, decrease, or remain the same as the system moves toward equilibrium at 900ºC.

We will use the reaction quotient, Q, to determine if a chemical reaction would be at equilibrium or not. The formula for Q is:

$\overline{){\mathbf{Q}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}}$

Depending on if Q is greater than or less than K our reaction will shift to attain equilibrium by reaching the equilibrium constant K: ###### Problem Details

At 900ºC, Kp = 1.04 for the reaction

CaCO3(s) ⇌ CaO(s) + CO2(g)

At a low temperature, dry ice (solid CO 2), calcium oxide, and calcium carbonate are introduced into a 50.0-L reaction chamber. The temperature is raised to 900ºC, 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 900ºC?

c. 0.14 g CaCO3, 5000 g CaO, PCO2 = 1.04 atm