hard · MCAT chem-phys
Solid calcium carbonate is heated in a sealed rigid container at constant temperature, establishing the heterogeneous equilibrium CaCO_3(s) rightleftharpoons CaO(s) + CO_2(g), with excess CaCO_3(s) and CaO(s) both present throughout.
If the container's volume is suddenly doubled at constant temperature, what happens to the equilibrium partial pressure of CO_2 once equilibrium is re-established?
- It halves, since the same moles of CO_2 now occupy twice the volume
- It returns to its original value, since K_p is fixed at a given temperature
- It doubles, since the container volume available to the gas has doubled
- It stays at the instantaneously lower value, since no further solid can decompose
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