At a certain temperature the vapor pressure of pure benzene (CH) is measured to be 0.19 atm. Suppose a solution is prepared by mixing 135. g of benzene and 113. g of acetyl bromide (CH₂COBr). Calculate the partial pressure of benzene vapor above this solution. Round your answer to 2 significant digits. Note for advanced students: you may assume the solution is ideal. Dat atm ☐ ☐x10 x

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Chapter1: Chemical Foundations
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At a certain temperature the vapor pressure of pure benzene (CH) is measured to be 0.19 atm. Suppose a solution is
prepared by mixing 135. g of benzene and 113. g of acetyl bromide (CH3COBr).
Calculate the partial pressure of benzene vapor above this solution. Round your answer to 2 significant digits.
Note for advanced students: you may assume the solution is ideal.
a
atm
П
☐x10
X
Transcribed Image Text:At a certain temperature the vapor pressure of pure benzene (CH) is measured to be 0.19 atm. Suppose a solution is prepared by mixing 135. g of benzene and 113. g of acetyl bromide (CH3COBr). Calculate the partial pressure of benzene vapor above this solution. Round your answer to 2 significant digits. Note for advanced students: you may assume the solution is ideal. a atm П ☐x10 X
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