What is the boiling point of a solution containing 0.144 g of eugenol dissolved in 10.0 g of benzene

The boiling point of solution is 80.32°C

Explanation:

To calculate the molality of solution, we use the equation:

Where,

= Given mass of solute (eugenol) = 0.144 g

= Molar mass of solute (eugenol) = 164.2 g/mol

= Mass of solvent (benzene) = 10.0 g

Putting values in above equation, we get:

To calculate the elevation in boiling point, we use the equation:

where,

= elevation in boiling point =

Boiling point of pure solution (benzene) = 80.1°C

i = Vant hoff factor = 1 (For non-electrolytes)

= molal boiling point elevation constant = 2.53°C/m

m = molality of solute = 0.088 m

Putting values in above equation, we get:

Hence, the boiling point of solution is 80.32°C

answers: to make sure that all of the broken pieces of tablet were added to the water, to allow for fair comparison of all three trials, with different particle sizes to avoid experimental error

substituting a hydrogen atom with a halogen in a hydrocarbon:

- the single bond remains single. a is wrong.

- the bond with hydrogen is as strong as with a halogen. c is wrong

- a hydrocarbon is saturated if there is no double bond. we do not know that so d is wrong.

- carbon will always have four valence electrons. e is wrong.

by elimination, the correct answer is b. the boiling point of the new compound increases.