When limestone (solid CaCO3) is heated, it decomposes into lime (solid Cao) and

Question

When limestone (solid CaCO3) is heated, it decomposes into lime (solid Cao) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete – the lime absorbs Co, from the air and turns back into hard, durable limestone. Suppose a limekiln of volume 850. L is pressurized with carbon dioxide gas to 14.9 atm, and heated to 920.0 °C. When the amount of Co, has stopped changing, it is found that 6.95 kg of CaCO3 have appeared. Calculate the pressure equilibrium constant K, this experiment suggests for the equilibrium between CaCO, and Cao at 920.0 °C. Round your answer to 2 significant digits. Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for K, does not match the accepted value. |K, =0 Ox109 *n?

Explanation / Answer

CaCO3 = CaO + CO2

Kp = P-CO2

all other are solids, no need to add thenm

Pinitial = 14.9 atm

PV = nRT

n = PV/(RT) = (14.9*850)/(0.082*(920+273))

n = 129.4645 mol of CO2 initially

then... after reaction

mass produced = 6.95 kg = 6950/100 = 69.5 mol of CaCO3 formed

then

CO2 rectedf =69.5 mol of CO2 lost

CO2 left = 129.4645 - 69.5 = 59.9645 mol of CO2 left

from:

P1/n1 = P2/n2

14.9/129.4645 = P2/59.9645

P2 = 59.9645 /129.4645 *14.9

P = 6.9012

Kp = P-CO2 ( in equilbirium )

Kp = 6.9012 atm

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