Question 13 A 1.28 M sample of hydrochloric acid degrades into 0.100 M of hydrogen gas and 0.150 M chlorine gas according to the following reaction: 2HCl (g) → H₂(g) + Cl₂ (9) At 793 K, the system will reach equilibrium. Determine the equilibrium concentration of HCI if the K = 0.136 at 793 K.

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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
icon
Related questions
icon
Concept explainers
Question

Please provide only typed answer solution no handwritten solution needed allowed 

Question 13
A 1.28 M sample of hydrochloric acid degrades into 0.100 M of hydrogen gas and 0.150 M chlorine
gas according to the following reaction:
2HCl (g) → H₂(g) + Cl₂ (g)
At 793 K, the system will reach equilibrium. Determine the equilibrium concentration of HCI if the
K = 0.136 at 793 K.
Question 14
The following reaction has an equilibrium constant of 8.20.
CH₁ (g) + H₂O (1) ⇒ CO(g) + 3H₂ (9)
Determine the difference between the equilibrium constant, K, and the reaction quotient, Q, when
[CH4} = 0.0274, [H} = 0.378 M, and [CO} = 0.254 M. Note: you are solving for K - Q, your answer
could be positive, negative, or zero.
Transcribed Image Text:Question 13 A 1.28 M sample of hydrochloric acid degrades into 0.100 M of hydrogen gas and 0.150 M chlorine gas according to the following reaction: 2HCl (g) → H₂(g) + Cl₂ (g) At 793 K, the system will reach equilibrium. Determine the equilibrium concentration of HCI if the K = 0.136 at 793 K. Question 14 The following reaction has an equilibrium constant of 8.20. CH₁ (g) + H₂O (1) ⇒ CO(g) + 3H₂ (9) Determine the difference between the equilibrium constant, K, and the reaction quotient, Q, when [CH4} = 0.0274, [H} = 0.378 M, and [CO} = 0.254 M. Note: you are solving for K - Q, your answer could be positive, negative, or zero.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps

Blurred answer
Knowledge Booster
Ionic Equilibrium
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY