A volume of 10⁻⁴ dm³ of liquid water is placed in a 1.0 dm³ container and kept at 300 K. At equilibrium, how many moles of water will be present in the vapour phase? (Given: vapour pressure of H2O at 300 K = 3170 Pa; R = 8.314 J K⁻¹ mol⁻¹)

Question

Accepted Answer

1.27 × 10⁻³ mol. The correct option is derived from applying the ideal gas law to the vapor pressure of water at the given temperature, which allows us to calculate the number of moles of water vapor that can exist in the container at equilibrium. By using the vapor pressure and the volume of the container, we find that the moles of water in the vapor phase is 1.27 × 10⁻³ mol.

A volume of 10⁻⁴ dm³ of liquid water is placed in a 1.0 dm³ container and kept at 300 K. At equilibrium, how many moles of water will be present in the vapour phase? (Given: vapour pressure of H2O at 300 K = 3170 Pa; R = 8.314 J K⁻¹ mol⁻¹)

Solution

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