A 2.0-mol sample of CaCO₃(s) is placed in a rigid 1.00-L reaction vessel from which all the air has been evacuated. The vessel is heated to 898°C, at which time the pressure of CO₂(g) in the vessel is constant at 1.00 atm, while some CaCO₃(s) remains in the vessel. 1.) Write the expression for Kp, the equilibrium constant for the reaction, and determine its value at 898°C. 2.)The experiment was repeated, but, this time, starting with a 4.0-mol sample of CaCO₃(s). On the following graph, draw a curve showing how the pressure of CO₂(g) would change over time as the vessel is heated to 898°C and equilibrium is established.