Question

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

Answer 1

0.22 atm.

Step-by-step explanation:

Acetyl bromide is a Chemical compound with molar mass of 122.95 g/mol and chemical formula of C2H3BrO. Acetyl bromide has a density of 1.66 g/cm³ and it is often classified as a volatile organic compound.

Chloroform is a Chemical compound with molar mass of 119.38 g/mol and chemical formula of CHCl₃.

So, let us delve right into the Calculations of the question above;

The number of moles of Acetyl bromide, C2H3BrO = mass/molar mass = 51.8/ 122.95 = 0.421 moles.

The number of moles of Chloroform, CHCl₃ = mass/ molar mass = 123/119.38 = 1.03 moles.

Total moles = 1.03 moles + 0.421 moles= 1.4513 moles.

Mole fraction of Acetyl bromide= 0.421 moles/1.4513 moles = 0.2901

Partial Pressure = 0.2901 × 0.75= 0.2176 atm.

= 0.22 atm.