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A student ran the following reaction in the laboratory at 743 K: N2(g) + 3H2(g) = 2NH3(g) When she introduced 3.39x102 moles of N,(g) and 5.98×102 moles of H,(g) into a 1.00 liter container, she found the equilibrium concentration of NH3(g) to be 8.32x10-4 M. Calculate the equilibrium constant, K. she obtained for this reaction. Kc =

A student ran the following reaction in the laboratory at 743 K: N2(g) + 3H2(g) = 2NH3(g) When she introduced 3.39x102 moles of N,(g) and 5.98×102 moles of H,(g) into a 1.00 liter container, she found the equilibrium concentration of NH3(g) to be 8.32x10-4 M. Calculate the equilibrium constant, K. she obtained for this reaction. Kc =

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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A student ran the following reaction in the laboratory at 743 K: N2(g) + 3H2(g) = 2NH3(g) When she introduced 3.39x1o2 moles of N-(g) and 5.98x102 moles of H2(g) into a 1.00 liter container, she found the equilibrium concentration of NH3(g) to be 8.32x104 M. Calculate the equilibrium constant, K, she obtained for this reaction. Kc =
Transcribed Image Text:A student ran the following reaction in the laboratory at 743 K: N2(g) + 3H2(g) = 2NH3(g) When she introduced 3.39x1o2 moles of N-(g) and 5.98x102 moles of H2(g) into a 1.00 liter container, she found the equilibrium concentration of NH3(g) to be 8.32x104 M. Calculate the equilibrium constant, K, she obtained for this reaction. Kc =
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