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.

Question

Chemistry

Rory Murphy

14 October, 08:51

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.

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Answers (1)

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Jorge · Answer 1

0.22 atm.

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.