Students were heating CaCO3 in an open container to produce CO2 gas,CaCO3(s) ⟶ CaO(s) + CO2(g)If we increase pressure on this system the:
Correct answer: D. System does not obey equilibrium rules
- A. Equilibrium will shift towards right
- B. Equilibrium will shift towards left
- C. Equilibrium will not be disturbed
- D. System does not obey equilibrium rules
Explanation
The correct answer is that the system does not obey equilibrium rules. Chemical equilibrium can only be established in a closed system where reactants and products are contained. In this scenario, the CaCO3 is heated in an open container, allowing the CO2 gas to escape. As a result, the system cannot reach equilibrium, as the continuous loss of CO2 gas prevents the establishment of a dynamic balance between reactants and products.All other options are incorrect because they assume that equilibrium can be achieved or disturbed in an open system, which is not possible. The nature of an open system prevents the maintenance of chemical equilibrium as it allows mass to be lost to the surroundings.
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About Chemical Equilibrium
Reversible reactions reach dynamic equilibrium when forward and reverse rates become equal, and Le Chatelier's principle predicts the effect of changing concentration, pressure or temperature. The chapter also covers solubility product, the common ion effect, buffer action and the conditions used in Haber's process, with equilibrium shifts distinguished from changes in the equilibrium constant.
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