Consider the following equilibrium: 2NH, (g) – N2 (g) + 3H, (g) AG° = 34. kJ Now suppose a reaction vessel is filled with 3.96 atm of ammonia (NH,) and 6.08 atm of nitrogen (N,) at 440. °C. Answer the following questions about this system: Under these conditions, will the pressure of NH, tend to rise or fall? O rise O fall Is it possible to reverse this tendency by adding H,? X. In other words, if you said the pressure of NH, will tend to rise, can that O yes be changed to a tendency to fall by adding H,? Similarly, if you said the O no pressure of NH, will tend to fall, can that be changed to a tendency to rise by adding H,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H, needed to reverse it. atm Round your answer to 2 significant digits.

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
Question
Consider the following equilibrium:
2NH; (g) – N, (g)+ 3H, (g)
AG = 34. kJ
Now suppose a reaction vessel is filled with 3.96 atm of ammonia (NH,) and 6.08 atm of nitrogen (N,) at 440. °C. Answer the following questions
about this system:
O rise
Under these conditions, will the pressure of NH, tend to rise or fall?
O fall
Is it possible to reverse this tendency by adding H,?
In other words, if you said the pressure of NH, will tend to rise, can that
yes
be changed to a tendency to fall by adding H,? Similarly, if you said the
O no
pressure of NH, will tend to fall, can that be changed to a tendency to
rise by adding H,?
If you said the tendency can be reversed in the second question, calculate
the minimum pressure of H, needed to reverse it.
atm
Round your answer to 2 significant digits.
Transcribed Image Text:Consider the following equilibrium: 2NH; (g) – N, (g)+ 3H, (g) AG = 34. kJ Now suppose a reaction vessel is filled with 3.96 atm of ammonia (NH,) and 6.08 atm of nitrogen (N,) at 440. °C. Answer the following questions about this system: O rise Under these conditions, will the pressure of NH, tend to rise or fall? O fall Is it possible to reverse this tendency by adding H,? In other words, if you said the pressure of NH, will tend to rise, can that yes be changed to a tendency to fall by adding H,? Similarly, if you said the O no pressure of NH, will tend to fall, can that be changed to a tendency to rise by adding H,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H, needed to reverse it. atm Round your answer to 2 significant digits.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps

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
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