Equilibrium constants can be measured for thedissociation of Lewis acid-base complexes such as thedimethyl ether complex of BF3, (CH3)20→BF3. Thevalue of K (here K,) for the reaction is 0.17 at 125 PC.(CH3)20 BF3 (g) 2 BF, (g) + (CHs)20(g)If 1.3 g of the complex is placed in a 75.5 mL flask at 125 degrees Celsius, what would the partialpressures (in atm) of the Lewis acid, Lewis base, and complex be? What would the total pressure(in atm) in the flask at equilibrium be?

Here i have solved the complete numerical using equilibrium constant

(CH3)20→BF3(g) 2 BF3 (g) + (CHs)20(g) If 1.3 g of the complex is placed in a 75.5 mL flask at 125 degrees Celsius, what would the partial pressures (in atm) of the Lewis acid, Lewis base, and complex be? What would the total pressure (in atm) in the flask at equilibrium be?

(CH3)20→BF3(g) 2 BF3 (g) + (CHs)20(g) If 1.3 g of the complex is placed in a 75.5 mL flask at 125 degrees Celsius, what would the partial pressures (in atm) of the Lewis acid, Lewis base, and complex be? What would the total pressure (in atm) in the flask at equilibrium be?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Equilibrium constants can be measured for the
dissociation of Lewis acid-base complexes such as the
dimethyl ether complex of BF3, (CH3)20→BF3. The
value of K (here K,) for the reaction is 0.17 at 125 PC.
(CH3)20 BF3 (g) 2 BF, (g) + (CHs)20(g)
If 1.3 g of the complex is placed in a 75.5 mL flask at 125 degrees Celsius, what would the partial
pressures (in atm) of the Lewis acid, Lewis base, and complex be? What would the total pressure
(in atm) in the flask at equilibrium be?

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