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Ethylene bromide C(2)H(4)Br(2), and 1,2 ...

Ethylene bromide `C_(2)H_(4)Br_(2)`, and 1,2 -dibromopropane,`C_(3)H_(6)Br_(2)`,form a series of ideal solutions over the whole range of composition. At `85^(@)C`, the vapour pressure of these two pure liquids are `173` and `127` torr, respectively.
. If `10.0 g` of ethylene bromide is dissolved in `80.0 g` of 1,2-dibromopropane, calculate the partial pressure of each component and teh total pressure of the solution at `85^(@)C`.
b. Calculate the mole fraction of ethylene bromide in the vapour in equilibrium with the above solution.
c. What would be the mole fraction of ethylene bromide in a solution at `85^(@)C` equilibrated with a `50 : 50` mole mixture in the vapour?

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AI Generated Solution

To solve the problem step by step, we will follow these calculations: ### Given Data: - **Ethylene bromide (C₂H₄Br₂)**: - Molecular weight = 188 g/mol - Vapor pressure at 85°C (P₀ₐ) = 173 torr - **1,2-Dibromopropane (C₃H₆Br₂)**: - Molecular weight = 202 g/mol ...
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