Homework Help is Here – Start Your Trial Now!
Science
Chemistry
2NH3(g) + 3O2(g) + 2CH4(g) 2HCN(g) + 6H2O(g) The above reaction is used in the industrial production of hydrogen cyanide. Consider the relevant thermodynamic data from the appendices of your text. (The tabulated values ΔH°f and S° are for 25°C. For the purposes of this question assume that ΔH° and ΔS° are invariant with temperature. This is not actually true but would generally be a reasonable approximation over "small" temperature ranges.) Answer the following practice questions: (a)Calculate ΔH° for this equation. (b)Calculate ΔS° for this equation. (c) Calculate ΔG° at 548°C, for this equation. (d) Are the following statements about this process True or False? The high temperature required for this process is needed for kinetic reasons. True of False? The equilibrium position for this reaction is further to the left at lower temperatures. True or False? This reaction is exothermic at room temperature. True or False? Thermodynamically, this reaction is spontaneous only above a certain temperature. True or False? At temperatures significantly lower than 1000°C this reaction is not spontaneous. True or False?

2NH3(g) + 3O2(g) + 2CH4(g) 2HCN(g) + 6H2O(g) The above reaction is used in the industrial production of hydrogen cyanide. Consider the relevant thermodynamic data from the appendices of your text. (The tabulated values ΔH°f and S° are for 25°C. For the purposes of this question assume that ΔH° and ΔS° are invariant with temperature. This is not actually true but would generally be a reasonable approximation over "small" temperature ranges.) Answer the following practice questions: (a)Calculate ΔH° for this equation. (b)Calculate ΔS° for this equation. (c) Calculate ΔG° at 548°C, for this equation. (d) Are the following statements about this process True or False? The high temperature required for this process is needed for kinetic reasons. True of False? The equilibrium position for this reaction is further to the left at lower temperatures. True or False? This reaction is exothermic at room temperature. True or False? Thermodynamically, this reaction is spontaneous only above a certain temperature. True or False? At temperatures significantly lower than 1000°C this reaction is not spontaneous. True or False?

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
2NH3(g) + 3O2(g) + 2CH4(g) 2HCN(g) + 6H2O(g)

The above reaction is used in the industrial production of hydrogen cyanide. Consider the relevant thermodynamic data from the appendices of your text. (The tabulated values ΔH°f and S° are for 25°C. For the purposes of this question assume that ΔH° and ΔS° are invariant with temperature. This is not actually true but would generally be a reasonable approximation over "small" temperature ranges.)

Answer the following practice questions:

(a)Calculate ΔH° for this equation.

(b)Calculate ΔS° for this equation.

(c) Calculate ΔG° at 548°C, for this equation.

(d) Are the following statements about this process True or False?

  • The high temperature required for this process is needed for kinetic reasons. True of False?
  • The equilibrium position for this reaction is further to the left at lower temperatures. True or False?
  • This reaction is exothermic at room temperature. True or False?
  • Thermodynamically, this reaction is spontaneous only above a certain temperature. True or False?
  • At temperatures significantly lower than 1000°C this reaction is not spontaneous. True or False?
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 4 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Thermodynamics
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