limestone decomposes at high temperatures. CaCO3(s),--->CaO(s)+CO2(g).At 1000 degrees C, Kp=3.87. If pure CaCO3 is placed in a 5 L flask and then heated to 1000 degrees celcius, what quantity of CaCO3 must decompose to acheive equlibrium pressure of CO2?

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Trinidad TremblayLv2

28 Sep 2019

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The dissociation of calcium carbonate has an equlibrium constant ofkp=1.16 at 800 degrees c. CaCO3(s)<---->CaO9s)+CO2(g).
a. what is the kc?
b.If you place 22.5 g of CaCO3 in a 9.56 L container at 800 degreescelcius, what is the pressure of Co2 in the container.?
c. What % of the original 22.5 g sample of CaCO3 remainsundercomposed at equilibrium?

For the reaction below, K_p = 1.16 at 800.°C.

CaCO₃(s) ⇌ CaO(s) + CO₂(g)

If a 20.0-g sample of CaCO₃ is put into a 10.0-L container and heated to 800.°C, what percentage by mass of the CaCO₃ will react to reach equilibrium?