Homework Help is Here – Start Your Trial Now!
Science
Chemistry
Ammonium iodide, a solid, decomposes to give NH3(g) and HI(g). At 406 °C, some NH4I(s) is placed in an evacuated container. A portion of it decomposes, and the total pressure at equilibrium is 1.07 atm. Extra NH3(g) is then injected into the container, and when equilibrium is reestablished, the partial pressure of NH3(9) is 1.37 atm. (a) Compute the equilibrium constant in terms of pressures, Kp, for the decomposition of ammonium iodide at 406 °C. (b) Determine the final partial pressure of HI(g) in the container. NH₂I(s) NH3(g) + HI(g) K= PHI atm

Ammonium iodide, a solid, decomposes to give NH3(g) and HI(g). At 406 °C, some NH4I(s) is placed in an evacuated container. A portion of it decomposes, and the total pressure at equilibrium is 1.07 atm. Extra NH3(g) is then injected into the container, and when equilibrium is reestablished, the partial pressure of NH3(9) is 1.37 atm. (a) Compute the equilibrium constant in terms of pressures, Kp, for the decomposition of ammonium iodide at 406 °C. (b) Determine the final partial pressure of HI(g) in the container. NH₂I(s) NH3(g) + HI(g) K= PHI 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
Ammonium iodide, a solid, decomposes to give NH3(9) and HI(g). At 406 °C, some NH4I(s) is placed in an evacuated container. A portion of it decomposes, and the total pressure at equilibrium is 1.07 atm. Extra NH3(9) is then injected into the container, and when equilibrium is reestablished, the partial pressure of NH3(9) is 1.37 atm. (a) Compute the equilibrium constant in terms of pressures, Kp, for the decomposition of ammonium iodide at 406 °C. (b) Determine the final partial pressure of HI(g) in the container. NH4I(s) NH3(g) + HI(g) PHI = atm
Transcribed Image Text:Ammonium iodide, a solid, decomposes to give NH3(9) and HI(g). At 406 °C, some NH4I(s) is placed in an evacuated container. A portion of it decomposes, and the total pressure at equilibrium is 1.07 atm. Extra NH3(9) is then injected into the container, and when equilibrium is reestablished, the partial pressure of NH3(9) is 1.37 atm. (a) Compute the equilibrium constant in terms of pressures, Kp, for the decomposition of ammonium iodide at 406 °C. (b) Determine the final partial pressure of HI(g) in the container. NH4I(s) NH3(g) + HI(g) PHI = atm
The reaction 2SO3(g)2SO₂(g) + O2(g) has an equilibrium constant Kp (in terms of pressures) at 877 °C of 2.74. Calculate the concentration of SO₂ that will be present at 877 °C in equilibrium with SO3 (at a concentration of 8.56x 10-3 mol L-¹) and O₂ (at a concentration of 8.10x10-3 mol L-1 Submit Answer 5 question attempts remaining [SO₂] =
Transcribed Image Text:The reaction 2SO3(g)2SO₂(g) + O2(g) has an equilibrium constant Kp (in terms of pressures) at 877 °C of 2.74. Calculate the concentration of SO₂ that will be present at 877 °C in equilibrium with SO3 (at a concentration of 8.56x 10-3 mol L-¹) and O₂ (at a concentration of 8.10x10-3 mol L-1 Submit Answer 5 question attempts remaining [SO₂] =
Expert Solution
Step 1

Given:

For equation:
NH4I(s)→ NH3(g) + HI(g) 

Total pressure  = 1.07 atm Partial pressure of NH3= 1.37 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