Consider the following equilibrium system: 2 NF3(g) <==> N2(g) + 3 F2(g) A 10.8 L evacuated flask is filled with 0.460 moles NF3(g). The temperature is then raised to 480K, where the decomposition of NF3(g) gas takes place to an appreciable extent. When equilibrium is established, the total pressure in the flask is 12.22 atm. What is the value of the equilibrium constant in terms of concentrations, Kc, at 480 K? 15 ΑΣΦ Submit Request Answer ?

Consider the following equilibrium system: 2 NF3(g) <==> N2(g) + 3 F2(g) A 10.8 L evacuated flask is filled with 0.460 moles NF3(g). The temperature is then raised to 480K, where the decomposition of NF3(g) gas takes place to an appreciable extent. When equilibrium is established, the total pressure in the flask is 12.22 atm. What is the value of the equilibrium constant in terms of concentrations, Kc, at 480 K? 15 ΑΣΦ Submit Request Answer ?

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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Question

Consider the following equilibrium system: 2 NF3(g) <==> N2(g) + 3 F₂(g)
A 10.8 L evacuated flask is filled with 0.460 moles NF3(g). The temperature is then raised to 480K, where the decomposition of NF3(g) gas
takes place to an appreciable extent. When equilibrium is established, the total pressure in the flask is 12.22 atm. What is the value of the
equilibrium constant in terms of concentrations, Kc, at 480 K?
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Step 2: Calculate Initial Pressure of Nitrogen Fluoride and Form ICE table:

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Step 3: Calculate the Equilibrium Pressures of Nitrogen and Fluorine:

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Step 4: Calculate Kp:

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Step 5: Calculate Kc:

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