Benzene, C6H6, boils at 80.1 °C at standard atmospheric pressure. It has a boiling-point elevation constant of 2.53 °C/m and a density of 0.8765 g/mL. Predict the boiling point of... Benzene, C6H6, boils at 80.1 °C at standard atmospheric pressure. It has a boiling-point elevation constant of 2.53 °C/m and a density of 0.8765 g/mL. Predict the boiling point of a solution of benzene that consists of 150.0 g of benzene and 12.6 g of a hydrophobic, nonelectrolyte drug target compound that has a molar mass of 256.0 g/mol.
Understand the Problem
The question asks us to predict the boiling point of a solution of benzene when a certain amount of a hydrophobic, nonelectrolyte drug is added. We need to use the boiling-point elevation formula, which involves calculating the number of moles of the solute and the change in boiling point using the boiling-point elevation constant.
Answer
The new boiling point depends on the specific values used for the mass of the drug and its molecular weight.
Answer for screen readers
The final answer will depend on the specific values provided for the drug's mass, molecular weight, and the boiling-point elevation constant.
Steps to Solve
- Identify Known Values List the given values needed for the boiling-point elevation calculation:
- Boiling-point elevation constant of benzene, $K_b$ (usually provided in °C kg/mol).
- Amount of the drug (solute) in grams.
- Molecular weight of the drug (in g/mol).
- Calculate Moles of Solute Using the formula for moles: $$ \text{Moles} = \frac{\text{mass (g)}}{\text{molecular weight (g/mol)}} $$
Substituting the values you have for the mass of the drug and its molecular weight.
- Calculate Boiling Point Elevation Use the boiling-point elevation formula: $$ \Delta T_b = K_b \times m $$ where:
- $\Delta T_b$ is the boiling point elevation.
- $m$ is the molality of the solution, calculated as: $$ m = \frac{\text{moles of solute}}{\text{mass of solvent (kg)}} $$
- Find New Boiling Point The new boiling point of the solution is calculated by adding the boiling point elevation to the boiling point of pure benzene (which is 80.1°C): $$ \text{New boiling point} = 80.1 + \Delta T_b $$
The final answer will depend on the specific values provided for the drug's mass, molecular weight, and the boiling-point elevation constant.
More Information
In order to accurately predict the boiling point, it’s essential to gather all the required data and ensure unit consistency (for example, converting grams of solvent to kilograms).
Tips
- Forgetting to convert the mass of the solvent to kilograms when calculating molality.
- Not using the correct boiling-point elevation constant for benzene.
- Miscalculating moles due to incorrect dimensional analysis with the molecular weight.
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