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Molecular bromine, Br2, dissociates at elevated temperatures into bromine atoms, Br. Br₂(g) → 2Br(g) A 7.130 L flask initially contains pure molecular bromine. The temperature is then raised to 1.600 × 10³ K. The total pressure of this equilibrium mixture at this elevated temperature is 1.000 atm. A spectroscopic analysis of this mixture showed that it contained 3.322 g of Br atoms. a. What are the total moles of gas in the container? b. What is the partial pressure of Br? mol Kp c. What is Kp for the dissociation of molecular bromine to bromine atoms? = atm

Molecular bromine, Br2, dissociates at elevated temperatures into bromine atoms, Br. Br₂(g) → 2Br(g) A 7.130 L flask initially contains pure molecular bromine. The temperature is then raised to 1.600 × 10³ K. The total pressure of this equilibrium mixture at this elevated temperature is 1.000 atm. A spectroscopic analysis of this mixture showed that it contained 3.322 g of Br atoms. a. What are the total moles of gas in the container? b. What is the partial pressure of Br? mol Kp c. What is Kp for the dissociation of molecular bromine to bromine atoms? = atm

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Molecular bromine, Br2, dissociates at elevated temperatures into bromine atoms, Br. Br₂ (g) = 2Br(g) A 7.130 L flask initially contains pure molecular bromine. The temperature is then raised to 1.600 × 10³ K. The total pressure of this equilibrium mixture at this elevated temperature is 1.000 atm. A spectroscopic analysis of this mixture showed that it contained 3.322 g of Br atoms. a. What are the total moles of gas in the container? b. What is the partial pressure of Br? mol Kp c. What is Kp for the dissociation of molecular bromine to bromine atoms? = atm
Transcribed Image Text:Molecular bromine, Br2, dissociates at elevated temperatures into bromine atoms, Br. Br₂ (g) = 2Br(g) A 7.130 L flask initially contains pure molecular bromine. The temperature is then raised to 1.600 × 10³ K. The total pressure of this equilibrium mixture at this elevated temperature is 1.000 atm. A spectroscopic analysis of this mixture showed that it contained 3.322 g of Br atoms. a. What are the total moles of gas in the container? b. What is the partial pressure of Br? mol Kp c. What is Kp for the dissociation of molecular bromine to bromine atoms? = atm
A mixture of 0.0255 mol phosphorus pentachloride, PC15, and 0.0855 mol helium gas, He, was placed in a 1.440 L flask and heated to 250.0°C. The phosphorus pentachloride decomposes at this temperature to give phosphorus trichloride, PC13, and chlorine gas, Cl₂. The helium gas is inert. PC15 (9) PC13 (9) + Cl₂ (9) a. What is the partial pressure of helium in this equilibrium mixture at 250.0°C? At equilibrium, the total pressure is found to be 3.630 atm. Partial pressure = b. What is Ke for the dissociation of PC15? Kc = Ke atm
Transcribed Image Text:A mixture of 0.0255 mol phosphorus pentachloride, PC15, and 0.0855 mol helium gas, He, was placed in a 1.440 L flask and heated to 250.0°C. The phosphorus pentachloride decomposes at this temperature to give phosphorus trichloride, PC13, and chlorine gas, Cl₂. The helium gas is inert. PC15 (9) PC13 (9) + Cl₂ (9) a. What is the partial pressure of helium in this equilibrium mixture at 250.0°C? At equilibrium, the total pressure is found to be 3.630 atm. Partial pressure = b. What is Ke for the dissociation of PC15? Kc = Ke atm
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