Enter your answer in the provided box. when 0.100 mol of caco3(s) and 0.100 mol of cao(s) are placed in an evacuated, sealed 10.0−l container and heated to 385 k, pco2 = 0.220 atm after equilibrium is established: caco3(s) ⇌ cao(s) + co2(g) an additional 0.240 atm of co2(g) is pumped in. what is the total mass (in g) of caco3 after equilibrium is reestablished?

Explanation:

Hi, step by step:

1) In equilibrium:

Assuming ideal gas:

In molarity:

2) Equilibrium constant:

For the given chemical reaction, the constant expression is:

Note: CaCO3 and CaO are not considered because they are in solid state

3) Concentrations in equilibrium:

Initial: 0.01 M of CaCO3 and 0.01 M of CaO

If 0.00697 M of dioxide where produced, also the same amount of CaO was produced. On the other side, 0.00697 M of CaCO3 where consumed. So:

Final: (0.01-0.00697) M of CaCO3, 0.00697 M of CO2 and (0.01+0.00697)M of CaO

4) Adding CO2

Aditional CO2: 0.24 atm:

The sistem will try to get back to equilibrium consuming those moles of CO2.

Following the inverse reaction, if 0.0076 M of CO2 are consumed, 0.0076 M of CaCO3 are produced:

The mass:

oxygen, selenium, tellurium, and polonium.

they're all from the same group as sulfur (group 16).