Answer :
The vapor pressure of the solution containing 24.6 g of camphor dissolved in 98.5 g of benzene would be lower than the vapor pressure of pure benzene.
To calculate the vapor pressure of the solution, we need to apply Raoult's law, which states that the vapor pressure of a solution is directly proportional to the mole fraction of the solvent present.
Step-by-step explanation:
1. Calculate the number of moles of camphor (C10H16O) and benzene (C6H6) using their respective molar masses.
Moles of camphor = mass of camphor / molar mass of camphor
Moles of benzene = mass of benzene / molar mass of benzene
2. Calculate the mole fraction of benzene.
Mole fraction of benzene = moles of benzene / (moles of benzene + moles of camphor)
3. Use Raoult's law to calculate the vapor pressure of the solution.
Vapor pressure of the solution = mole fraction of benzene * vapor pressure of pure benzene
Note: The vapor pressure of pure benzene is given as 100.0 mmHg at 26.1 °C.
In the description, I have provided the general steps to calculate the vapor pressure of the solution based on Raoult's law.
However, I cannot provide the exact numerical calculation without the values of the molar masses of camphor and benzene.
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