At a certain temperature the vapor pressure of pure acetyl bromide CH3COBr is measured to be 467.torr. Suppose a solution is prepared by mixing 72.6g of acetyl bromide and 144.g of chloroform CHCl3.Calculate the partial pressure of acetyl bromide vapor above this solution. Round your answer to 3 significant digits.Note for advanced students: you may assume the solution is ideal.

To calculate the partial pressure of acetyl bromide vapor above the solution, we need to use Raoult's Law, which states that the partial pressure of a component in an ideal solution is equal to the vapor pressure of the pure component multiplied by its mole fraction in the solution.

Step 1: Calculate the moles of acetyl bromide (CH3COBr).

• Molar mass of CH3COBr = 12.01 (C) + 1.01 (H) * 3 + 12.01 (C) + 16.00 (O) + 79.90 (Br) = 122.93 g/mol
• Moles of CH3COBr = mass / molar mass = 72.6 g / 122.93 g/mol = 0.591 moles

Step 2: Calculate the moles of chloroform (CHCl3).

• Molar mass of CHCl3 = 12.01 (C) + 1.01 (H) + 35.45 (Cl) * 3 = 119.37 g/mol
• Moles of CHCl3 = mass / molar mass = 144 g / 119.37 g/mol = 1.206 moles

Step 3: Calculate the total moles in the solution.

• Total moles = moles of CH3COBr + moles of CHCl3 = 0.591 + 1.206 = 1.797 moles

Step 4: Calculate the mole fraction of acetyl bromide (CH3COBr).

• Mole fraction of CH3COBr = moles of CH3COBr / total moles = 0.591 / 1.797 = 0.329

Step 5: Calculate the partial pressure of acetyl bromide using Raoult's Law.

• Partial pressure of CH3COBr = mole fraction of CH3COBr * vapor pressure of pure CH3COBr
• Partial pressure of CH3COBr = 0.329 * 467 torr = 153.783 torr

Step 6: Round the answer to 3 significant digits.

• Partial pressure of CH3COBr = 154 torr

Therefore, the partial pressure of acetyl bromide vapor above the solution is 154 torr.