Ask a New Question
Menu

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

CaCO3(s) CaO(s) + CO2(g)
If a 25.0-g sample of CaCO3 is put into a 10.2-L container and heated to 800.°C, what percent of the CaCO3 will react to reach
equilibrium?

2 answers

CaCO3(s) ==> CaO(s) + CO2
I...25.0.......0.........0
C.......................x
E........................x

Kp = pCO2 = 1.16
Therefore, p CO2 = 1.16 atm. Plug that into PV = nRT and solve for n.
Convert 25.0 g CaCO3 to mols, then calculate the percent decomposed.
34%
Similar Questions
    1. answers icon 2 answers
  2. Reaction:CaCO3 + 2 HCl -> CaCl2 + CO2 + H2O Calculate the molarity of hydrochloric acid solution if an initial mass of 4.568g of
    1. answers icon 2 answers
  3. For the reaction below, Kp = 1.16 at 800.°C.CaCO3(s) CaO(s) + CO2(g) If a 21.7-g sample of CaCO3 is put into a 10.6 L container
    1. answers icon 1 answer
  4. For the reaction below, Kp = 1.16 at 800.°C.CaCO3(s) CaO(s) + CO2(g) If a 21.7-g sample of CaCO3 is put into a 10.6 L container
    1. answers icon 1 answer
more similar questions