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Answer :
Final answer:
The vapor pressure of both beaker (i) and beaker (ii) will be equal. So the correct option is c).
Explanation:
In a closed container, when two beakers are placed together, the vapor pressure is determined by the nature of the solvent, not the presence of a solute. Raoult's law states that the vapor pressure of a solution is directly proportional to the mole fraction of the solvent. In beaker (i), containing only a pure volatile solvent, the mole fraction of the solvent is 1, and in beaker (ii), with a volatile solvent and non-volatile solute, the mole fraction of the solvent is still 1, as the solute does not contribute to the vapor pressure. Therefore, the vapor pressure of both beaker (i) and beaker (ii) will be equal, as they both have the same solvent.
This equalization occurs because the addition of a non-volatile solute does not affect the vapor pressure of the solvent. The solute may change other properties like boiling point or freezing point, but vapor pressure remains unaffected according to Raoult's law.
In summary, the vapor pressure in both beakers is solely determined by the pure volatile solvent, leading to an equal vapor pressure in both beakers when placed together in a closed container. Therefore, the correct option is c).
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