Jawaban:

To solve this problem, we need to use Raoult's Law, which states that the vapor pressure of a solution is equal to the mole fraction of the solvent times the vapor pressure of the pure solvent.

First, we need to calculate the mole fraction of benzene in the solution. We can do this using the formula:

mole fraction = moles of benzene / total moles of solution

To calculate moles of benzene, we need to convert the given mass to moles using the molar mass of benzene:

molar mass of benzene (C6H6) = 78.11 g/mol

moles of benzene = mass of benzene / molar mass of benzene

= 98.5 g / 78.11 g/mol

= 1.259 mol

To calculate the total moles of the solution, we need to add the moles of benzene to the moles of camphor:

moles of camphor = mass of camphor / molar mass of camphor

= 24.6 g / 152.23 g/mol

= 0.162 mol

total moles of solution = moles of benzene + moles of camphor

= 1.259 mol + 0.162 mol

= 1.421 mol

Now we can calculate the mole fraction of benzene:

mole fraction of benzene = moles of benzene / total moles of solution

= 1.259 mol / 1.421 mol

= 0.886

Next, we can use Raoult's Law to calculate the vapor pressure of the solution:

vapor pressure of solution = mole fraction of benzene x vapor pressure of pure benzene

We are given that the vapor pressure of pure benzene is 100.0 mmHg. Substituting the values we have calculated, we get:

vapor pressure of solution = 0.886 x 100.0 mmHg

= 88.6 mmHg

Therefore, the vapor pressure of the solution containing camphor and benzene is 88.6 mmHg.