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2.50 mol of HI(g) sealed in a 10.32 L volume forms H2(g) and I2(g) at 25 °C.  Use K = 1.26 × 10–3 to find all [conc]eq in this equilibrium mixture: 2HI(g) <-->  H2(g) + I2(g) Set up an ICE table:   [HI]  [H2]  [I2]  Init  Change  Eqºm   Use other given data to calculate the unknown: k = x2/____ =1.26×10-3 x/______ = ________ [H2]eq = _______ M  [I2]eq = _______ M [HI]eq = _______ M

2.50 mol of HI(g) sealed in a 10.32 L volume forms H2(g) and I2(g) at 25 °C.  Use K = 1.26 × 10–3 to find all [conc]eq in this equilibrium mixture: 2HI(g) <-->  H2(g) + I2(g) Set up an ICE table:   [HI]  [H2]  [I2]  Init  Change  Eqºm   Use other given data to calculate the unknown: k = x2/____ =1.26×10-3 x/______ = ________ [H2]eq = _______ M  [I2]eq = _______ M [HI]eq = _______ M

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter12: Gaseous Chemical Equilibrium
Section: Chapter Questions
Problem 36QAP: At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s),...
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2.50 mol of HI(g) sealed in a 10.32 L volume forms H2(g) and I2(g) at 25 °C.  Use K = 1.26 × 10–3 to find all [conc]eq in this equilibrium mixture:

2HI(g) <-->  H2(g) + I2(g)

Set up an ICE table:

  [HI]  [H2]  [I2] 

Init 

Change 

Eqºm  

Use other given data to calculate the unknown:

k = x2/____ =1.26×10-3

x/______ = ________

[H2]eq = _______ M  [I2]eq = _______ M

[HI]eq = _______ M

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