Step 1. Calculate for the molarity of CO2 at equilibrium
Step 2. Setup the Keq expression
Recall that the equilibrium constant is the ratio of the products and reactants. We use Kp when dealing with pressure and Kc when dealing with concentration:
Recall CaCO3 and CaO are not included in the Kp expression since they are both in solid state
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 0.300 atm of CO2(g) is pumped in. What is the total mass (in g) of CaCO 3 after equilibrium is re-established?
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Based on our data, we think this problem is relevant for Professor Heiden's class at Michigan Technological University.
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Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.