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A chemist placed a mixture of CO₂ (g) and CF4 (9) into a flask at a particular temperature. These gases react: CO₂ (g) + CF4 (g) = 2COF₂ (g) After this mixture came to equilibrium, she found that it contained 0.45 mole fraction of CF4 and 0.12 mole fraction of COF2. Calculate K₂ at this temperature for this reaction. Kp =

A chemist placed a mixture of CO₂ (g) and CF4 (9) into a flask at a particular temperature. These gases react: CO₂ (g) + CF4 (g) = 2COF₂ (g) After this mixture came to equilibrium, she found that it contained 0.45 mole fraction of CF4 and 0.12 mole fraction of COF2. Calculate K₂ at this temperature for this reaction. Kp =

Chemistry
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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A chemist placed a mixture of CO₂ (g) and CF4 (9) into a flask at a particular temperature. These gases react: CO2 (g) + CF4 (9) ⇒ 2COF2 (g) After this mixture came to equilibrium, she found that it contained 0.45 mole fraction of CF4 and 0.12 mole fraction of COF2. Calculate K₂ at this temperature for this reaction. Kp =
Transcribed Image Text:A chemist placed a mixture of CO₂ (g) and CF4 (9) into a flask at a particular temperature. These gases react: CO2 (g) + CF4 (9) ⇒ 2COF2 (g) After this mixture came to equilibrium, she found that it contained 0.45 mole fraction of CF4 and 0.12 mole fraction of COF2. Calculate K₂ at this temperature for this reaction. Kp =
A chemist wants to prepare phosgene, COCl2, by the following reaction: CO(g) + Cl₂ (g) = COCl₂ (g) He places 4.10 g of chlorine, Cl2, and an equal molar amount of carbon monoxide, CO, into a 10.00 L reaction vessel at 395°C. After the reaction comes to equilibrium, he adds another 4.10 g of chlorine to the vessel in order to push the reaction to the right to get more product. What is the partial pressure of phosgene when the reaction again comes to equilibrium? Ke 1.23 × 10³ = Partial pressure = atm
Transcribed Image Text:A chemist wants to prepare phosgene, COCl2, by the following reaction: CO(g) + Cl₂ (g) = COCl₂ (g) He places 4.10 g of chlorine, Cl2, and an equal molar amount of carbon monoxide, CO, into a 10.00 L reaction vessel at 395°C. After the reaction comes to equilibrium, he adds another 4.10 g of chlorine to the vessel in order to push the reaction to the right to get more product. What is the partial pressure of phosgene when the reaction again comes to equilibrium? Ke 1.23 × 10³ = Partial pressure = atm
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