In the phase diagram, the regions have to be labeled. Concept Introduction: Phase diagrams are the one where the pressure is plotted against temperature of the substance. Stability of the physical state for the substance can be obtained. The equilibrium between two phases if it exists can be inferred. Triple point for the substance is shown and also the melting, boiling point.

Question

Using reaction free energy to predict equilibrium composition Consider the following equilibrium: 2NO2 (g) = N2O4(g) AGº = -5.4 kJ Now suppose a reaction vessel is filled with 4.53 atm of dinitrogen tetroxide (N2O4) at 279. °C. Answer the following questions about this system: Under these conditions, will the pressure of N2O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO2? In other words, if you said the pressure of N2O4 will tend to rise, can that be changed to a tendency to fall by adding NO2? Similarly, if you said the pressure of N2O4 will tend to fall, can that be changed to a tendency to '2' rise by adding NO2? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO 2 needed to reverse it. Round your answer to 2 significant digits. 00 rise ☐ x10 fall yes no ☐ atm G Ar 1

Answer 1

Question

Chapter 11, Problem 11.44QE

(a)

Interpretation Introduction

Interpretation:

In the phase diagram, the regions have to be labeled.

Concept Introduction:

Phase diagrams are the one where the pressure is plotted against temperature of the substance.

Stability of the physical state for the substance can be obtained.

The equilibrium between two phases if it exists can be inferred.

Triple point for the substance is shown and also the melting, boiling point.

(b)

Interpretation Introduction

Interpretation:

The phase or phases that is present in the points labeled as G, H, J, and K has to be identified.

Concept Introduction:

Refer part (a).

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Using reaction free energy to predict equilibrium composition Consider the following equilibrium: 2NO2 (g) = N2O4(g) AGº = -5.4 kJ Now suppose a reaction vessel is filled with 4.53 atm of dinitrogen tetroxide (N2O4) at 279. °C. Answer the following questions about this system: Under these conditions, will the pressure of N2O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO2? In other words, if you said the pressure of N2O4 will tend to rise, can that be changed to a tendency to fall by adding NO2? Similarly, if you said the pressure of N2O4 will tend to fall, can that be changed to a tendency to '2' rise by adding NO2? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO 2 needed to reverse it. Round your answer to 2 significant digits. 00 rise ☐ x10 fall yes no ☐ atm G Ar 1

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