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Consider the following reaction: 2NH3(9) N₂(g) + 3H₂(9) If 1.54x10-3 moles of NH3(g), 0.549 moles of N₂, and 0.352 moles of H₂ are at equilibrium in a 19.7 L container at 792 K, the value of the equilibrium constant, K, is

Consider the following reaction: 2NH3(9) N₂(g) + 3H₂(9) If 1.54x10-3 moles of NH3(g), 0.549 moles of N₂, and 0.352 moles of H₂ are at equilibrium in a 19.7 L container at 792 K, the value of the equilibrium constant, K, is

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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Consider the following reaction: 2NH3(g) N₂(g) + 3H₂(g) If 1.54x10-3 moles of NH3(g), 0.549 moles of N₂, and 0.352 moles of H₂ are at equilibrium in a 19.7 L container at 792 K, the value of the equilibrium constant, K, is
Transcribed Image Text:Consider the following reaction: 2NH3(g) N₂(g) + 3H₂(g) If 1.54x10-3 moles of NH3(g), 0.549 moles of N₂, and 0.352 moles of H₂ are at equilibrium in a 19.7 L container at 792 K, the value of the equilibrium constant, K, is
Expert Solution
Step 1

The equilibrium constant is 

Kc tell about the Concentration of ratio of products and reactant 

The Concentration express in Mole/ litre 

Given Concentration at equilibrium 

N2 = 0.549/19.7      mole/ litre 

H2 =. 352/19.7       mole/litre

NH3 = 1.54 ×10^3 mole/litre 

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