Homework Help is Here – Start Your Trial Now!
Science
Chemistry
The equilibrium constant in terms of pressures, Kp, for the reaction NH3(g) + HCl(g) NH4Cl(s) at 340 °C is 4.00. (a) If the partial pressure of ammonia is PNH, = 0.840 atm and solid ammonium chloride is present, what is the equilibrium partial pressure of hydrogen chloride at 340 °C? PHCI = atm

The equilibrium constant in terms of pressures, Kp, for the reaction NH3(g) + HCl(g) NH4Cl(s) at 340 °C is 4.00. (a) If the partial pressure of ammonia is PNH, = 0.840 atm and solid ammonium chloride is present, what is the equilibrium partial pressure of hydrogen chloride at 340 °C? PHCI = atm

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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
See similar textbooks
icon
Related questions
Question
The equilibrium constant in terms of pressures, Kp, for the reaction NH3(g) + HCl(g) 2NH4CI(S) at 340 °C is 4.00. (a) If the partial pressure of ammonia is PNH3 = 0.840 atm and solid ammonium chloride is present, what is the equilibrium partial pressure of hydrogen chloride at 340 °C? PHCI = (b) An excess of solid NH4Cl is added to a container filled with NH3 at 340 °C and a pressure of 1.34 atm. Calculate the pressures of NH3(9) and HCI(g) reached at equilibrium. PNH3 = atm PHCI = atm atm
Transcribed Image Text:The equilibrium constant in terms of pressures, Kp, for the reaction NH3(g) + HCl(g) 2NH4CI(S) at 340 °C is 4.00. (a) If the partial pressure of ammonia is PNH3 = 0.840 atm and solid ammonium chloride is present, what is the equilibrium partial pressure of hydrogen chloride at 340 °C? PHCI = (b) An excess of solid NH4Cl is added to a container filled with NH3 at 340 °C and a pressure of 1.34 atm. Calculate the pressures of NH3(9) and HCI(g) reached at equilibrium. PNH3 = atm PHCI = atm atm
The equilibrium constant in terms of pressures for the reduction of tungsten (VI) oxide to tungsten at 25 °C is Kp = 21.1, corresponding to the reaction WO3(s) + 3CO(g) 2W(s) + 3CO₂(g) If the total pressure of an equilibrium system at 25 °C is 2.96 atm, calculate the partial pressures of CO(g) and CO₂(g). Pco= PCO₂ atm atm
Transcribed Image Text:The equilibrium constant in terms of pressures for the reduction of tungsten (VI) oxide to tungsten at 25 °C is Kp = 21.1, corresponding to the reaction WO3(s) + 3CO(g) 2W(s) + 3CO₂(g) If the total pressure of an equilibrium system at 25 °C is 2.96 atm, calculate the partial pressures of CO(g) and CO₂(g). Pco= PCO₂ atm atm
Expert Solution
Step 1 Calculation of required value for the first equilibrium reaction

Given equilibrium reaction ;

                        NH3 (g)  +  HCl (g)  ⇔NH4Cl (s)

                         Kp of the reaction at 340 oC = 4.00

 (a)  Partial pressure of NH3 (pNH3) = 0.840 atm

       Now, the expression of Kp for the given equilibrium reaction is ;

                                     Kp=1pNH3×pHCl              ( Since NH4Cl is solid and so its fugacity is equal to unity)

                               ⇒ 4 = 10.840 ×pHCl

                               ⇒pHCl = 10.840 ×4

                               ⇒pHCl = 0.298 atm

Hence, the equilibrium partial pressure of hydrogen chloride at 340 oC is 0.298 atm

steps

Step by step

Solved in 2 steps

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
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
SEE MORE TEXTBOOKS