Question
Asked Nov 30, 2019
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The standard reaction Gibbs energy of the isomerization of borneol (CioH17OH) to
isoborneol (C10H7OH) in the gas phase at 503 K is +9.4 kJ/mol. Calculate the reaction
Gibbs energy in a mixture consisting of 0.15 mol of borneol and 0.30 mol of isoborneol
when the total pressure is 600 torr
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The standard reaction Gibbs energy of the isomerization of borneol (CioH17OH) to isoborneol (C10H7OH) in the gas phase at 503 K is +9.4 kJ/mol. Calculate the reaction Gibbs energy in a mixture consisting of 0.15 mol of borneol and 0.30 mol of isoborneol when the total pressure is 600 torr

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Expert Answer

Step 1

Given:

Standard Gibbs energy (ΔGo) = +94 KJ/mol

Temperature (T) = 503 K

Total pressure Ptotal = 600 torr.

Number of moles of borneol nB = 0.15 mol

Number of moles of Isoborneol nI = 0.30 mol

Step 2

Calculation of mole fraction of borneol:

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Пв Хв n + Пв 0.15 mol Хв 0.15 mol0.30 mol Хв — 0.3334

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Step 3

Calculation for partial pressure ...

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Рв — Хв X Рotal Рв — 0.3334 х 600 torr Рв 3 200 torr Protal 3D Рв + P Р — PРrotal - Pв P 600 torr 200 torr = 400 torr

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