Homework Help is Here – Start Your Trial Now!
Science
Chemistry
4. Consider an equilibrium mixture of the following chemical reaction : Fe"(aq) + SCN (aq) Fe(SCN)"(aq) yellow colourless deep red (a) Write an expression for the equilibrium constant Kc for the reaction. (b) At a certain temperature, the equilibrium constant Kc for the reaction is 1.08 x 10° dm mol*. The equilibrium mixture is prepared by mixing 20.0 cm of 0.030 M Fe(NO3)3(aq) with 10.0 cm of 0.030 M KSCN(aq) in an acidic medium. Calculate the concentration of Fe(SCN)²*(aq) in the equilibrium mixture at that temperature. (c) It is known that the equilibrium constant Kc increases when temperature increases. Suggest and explain whether the enthalpy change of the reaction is positive, negative or zero.

4. Consider an equilibrium mixture of the following chemical reaction : Fe"(aq) + SCN (aq) Fe(SCN)"(aq) yellow colourless deep red (a) Write an expression for the equilibrium constant Kc for the reaction. (b) At a certain temperature, the equilibrium constant Kc for the reaction is 1.08 x 10° dm mol*. The equilibrium mixture is prepared by mixing 20.0 cm of 0.030 M Fe(NO3)3(aq) with 10.0 cm of 0.030 M KSCN(aq) in an acidic medium. Calculate the concentration of Fe(SCN)²*(aq) in the equilibrium mixture at that temperature. (c) It is known that the equilibrium constant Kc increases when temperature increases. Suggest and explain whether the enthalpy change of the reaction is positive, negative or zero.

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.41PAE: Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go...
See similar textbooks
icon
Related questions
Question
100%
4. Consider an equilibrium mixture of the following chemical reaction : Fe"(aq) + SCN (aq) – Fe(SCN)³"(aq) yellow colourless deep red (a) Write an expression for the equilibrium constant Kc for the reaction. (b) At a certain temperature, the equilibrium constant Kc for the reaction is 1.08 x 10° dm³ mol1. The equilibrium mixture is prepared by mixing 20.0 cm³ of 0.030 M Fe(NO3)3(aq) with 10.0 cm³ of 0.030 M KSCN(aq) in an acidic medium. Calculate the concentration of Fe(SCN)²*(aq) in the equilibrium mixture at that temperature. (c) It is known that the equilibrium constant Kc increases when temperature increases. Suggest and explain whether the enthalpy change of the reaction is positive, negative or zero. (d) When a little amount of Na,SO3(s) is added to the equilibrium mixture, the colour of the mixture becomes paler. Explain this observation.
Transcribed Image Text:4. Consider an equilibrium mixture of the following chemical reaction : Fe"(aq) + SCN (aq) – Fe(SCN)³"(aq) yellow colourless deep red (a) Write an expression for the equilibrium constant Kc for the reaction. (b) At a certain temperature, the equilibrium constant Kc for the reaction is 1.08 x 10° dm³ mol1. The equilibrium mixture is prepared by mixing 20.0 cm³ of 0.030 M Fe(NO3)3(aq) with 10.0 cm³ of 0.030 M KSCN(aq) in an acidic medium. Calculate the concentration of Fe(SCN)²*(aq) in the equilibrium mixture at that temperature. (c) It is known that the equilibrium constant Kc increases when temperature increases. Suggest and explain whether the enthalpy change of the reaction is positive, negative or zero. (d) When a little amount of Na,SO3(s) is added to the equilibrium mixture, the colour of the mixture becomes paler. Explain this observation.
Expert Solution
steps

Step by step

Solved in 4 steps with 3 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Chemical 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.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry for Engineering Students
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
Introduction to General, Organic and Biochemistry
Introduction to General, Organic and Biochemistry
Chemistry
ISBN:
9781285869759
Author:
Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:
Cengage Learning
Chemistry: Principles and Practice
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
SEE MORE TEXTBOOKS