Answer:
10.32g
Explanation:
First thing's first, lets bring out the balanced chemical equation representing the reaction.
CaCO3(s) ⇄ CaO(s) + CO2(g)
From the question;
reaction constant K = [CO2(g)] = 0.220 atm.
To obtain number of moles of CO2, using ideal gas fomula, we have;
n = PV/RT = 0.220*10 / (0.08206*385) = 0.0696(mol)
From the stoichiometry of the equation above;
This is the amount of CaCO3 which has been converted to CaO before additional 0.230 atm CO2(g) is added.
After the additional 0.230 atm CO2(g), the equilibrium CO2 pressure is still 0.220 atm. Therefore all this additional CO2 would completely convert to CaCO3:
n = PV/RT = 0.230*10.0/(0.08206*385) = 0.0728 (mol)
Hence the total CaCO3 after equilibrium is reestablished is:
0.100 - 0.0696 + 0.0728 (mol) = 0.1032 mol
Mass = Number of moles * Molar mass
Mass = 0.1032 * 100 = 10.32g
