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: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 61QRT

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