Question

When limestone (CaCO₃ solid) is heated, it decomposes into lime (CaO solid) and carbon dioxide gas. Suppose a limekiln of volume 400L is pressurized with carbon dioxide gas to 14.0 atm and heated to 710.0°C. Calculate the pressure equilibrium constant this experiment suggests for the equilibrium between CaCO₃ and CaO at 710°C.

a) Kₚ = 0.0023

b) Kₚ = 0.0354

c) Kₚ = 0.0897

d) Kₚ = 0.2046

Answer 1

The equilibrium constant for the decomposition of calcium carbonate into calcium oxide and carbon dioxide at 710°C can be calculated using the ideal gas law to find the number of moles of CO2 and applying the equilibrium expression for Kp, which is the partial pressure of CO2.

Step-by-step explanation:

The decomposition of limestone (calcium carbonate, CaCO₃) into lime (calcium oxide, CaO) and carbon dioxide (CO₂) when heated can be characterized by an equilibrium constant.

At 710.0°C, given that the volume of the limekiln is 400L and the carbon dioxide gas is at a pressure of 14.0 atm, we can calculate the pressure equilibrium constant (Kp) for this reaction using the ideal gas law (PV=nRT) to find the number of moles of CO₂ and then applying the equilibrium expression for Kp, which in this case is simply the partial pressure of CO₂ since solids like CaCO₃ and CaO don't appear in the expression.

To answer this question correctly, it requires a calculation based on these principles, referencing the student's coursework or textbook as needed for the appropriate equations.