1) H, 2 H,S e) Keq= 14 (s). (g) (g) 0.60 moles of H, and 1.4 moles of S are placed into a 2.0L flask and allowed to reach equilibrium. Calculate the [H,] at equilibrium.
1) H, 2 H,S e) Keq= 14 (s). (g) (g) 0.60 moles of H, and 1.4 moles of S are placed into a 2.0L flask and allowed to reach equilibrium. Calculate the [H,] at equilibrium.
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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![### Chemical Equilibrium Problems
**Problem 1:**
For the equilibrium reaction:
\[ \text{H}_2 (\text{g}) + \text{S} (\text{s}) \rightleftharpoons \text{H}_2\text{S} (\text{g}) \]
where \( \text{Keq} = 14 \).
Two reactants, 0.60 moles of \( \text{H}_2 \) and 1.4 moles of \( \text{S} \), are placed into a 2.0 L flask and allowed to reach equilibrium. Calculate the concentration of \( [\text{H}_2] \) at equilibrium.
**Problem 2:**
For the reaction:
\[ 2\text{HI} (\text{g}) \rightleftharpoons \text{H}_2 (\text{g}) + \text{I}_2 (\text{g}) \]
where \( \text{Keq} = 0.0183 \).
If 3.0 moles of \( \text{HI} \) are placed in a 5.00 L vessel and allowed to reach equilibrium, what is the equilibrium concentration of \( \text{H}_2 \)?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F63a27622-a493-4bf8-aa5e-97adfc7108ed%2Fce7d6f2f-85f7-4859-8534-6468da1b47ed%2Fxpwb29o_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemical Equilibrium Problems
**Problem 1:**
For the equilibrium reaction:
\[ \text{H}_2 (\text{g}) + \text{S} (\text{s}) \rightleftharpoons \text{H}_2\text{S} (\text{g}) \]
where \( \text{Keq} = 14 \).
Two reactants, 0.60 moles of \( \text{H}_2 \) and 1.4 moles of \( \text{S} \), are placed into a 2.0 L flask and allowed to reach equilibrium. Calculate the concentration of \( [\text{H}_2] \) at equilibrium.
**Problem 2:**
For the reaction:
\[ 2\text{HI} (\text{g}) \rightleftharpoons \text{H}_2 (\text{g}) + \text{I}_2 (\text{g}) \]
where \( \text{Keq} = 0.0183 \).
If 3.0 moles of \( \text{HI} \) are placed in a 5.00 L vessel and allowed to reach equilibrium, what is the equilibrium concentration of \( \text{H}_2 \)?
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