**Question 9**Regarding the following reaction at constant temperature, calculate the ratio of Kx at a total pressure of 5.0 bar to that at 1.5 bar. Please enter your answer with one decimal. For example, 0.567 is written as 0.6.\[ \text{H}_2\text{CO (g)} = \text{CO (g)} + \text{H}_2\text{ (g)}. \][Text box for answer entry]

Write the reaction as follows: H2COg ↔COg +H2g Equilibrium constant is defined as the ratio of…

Answered: QUESTION 9 Regarding the following…

Introduction to Chemical Engineering Thermodynamics

8th Edition

ISBN:9781259696527

Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Chapter1: Introduction

Section: Chapter Questions

Problem 1.1P

See similar textbooks

Similar questions

As we discussed in class, although low temperatures favor the formation of ammonia in Haber process, in practice higher temperatures, on the order of 450 ◦C, are used. (a) Repeat the computation of the relative reaction extent that we did in the class (or just use the formula for reaction extent given in the notes) at T = 450 ◦C and constant overall pressure of 1 bar and 200 bar. Assume that the reaction enthalpy and entropy do not depend on the temperature. You will need to consult thermodynamic tables to determine the equilibrium constant at this temperature. (b) Instead of keeping the overall pressure constant, assume that the reaction occurs in a fixed-volume container (at const T). Assuming that 3/2 mol of H2 and 1/2 mol of N2 are mixed at T = 450 ◦Cand p = 200 bar, determine the reaction extent at equilibrium. Note that p will now depend on the reaction extent, hence the relation between the reaction extent and Kp must be re-derived.
4.) At 650 C the reaction below has a Keq value of 0.843. If 2 mol of both hydrogen and carbon dioxide gases are placed in a 4L container. What will be the equilibrium calculations of all four gases? CO2(g) + H2(g) –> CO(g) + H2O(g)
2. Consider the following reaction: CO) +=O=COz) s) Find AH (kJ/mol) of the reaction at 298 K and 1 bar (b) ›) Determine the spontaneity of the reaction in a furnace operating at 2000 K where the partial pressures of the compounds are: Compound iP (bar) CO(R) O₂(g) CO2(g) Consider that for this reaction AG2000k = -111 kJ/mol 0.05 2.00 2.50
Calculate the Gibbs free energy of fusion (melting) for water [in J/mol] at T = 0°C at 15.0 bar noting that it is zero at 1.0 bar. Assume the densities of the two phases are 1.000 g/cc (liquid) and 0.9150 g/cc (solid).
2. Consider the following reaction: +02(8) ² = CO2(g) 3) Find AH (kJ/mol) of the reaction at 298 K and 1 bar CO(g) +
Consider the reaction: N₂(g) + O2(g) → 2NO(g) Using standard absolute entropies at 298 K, calculate the entropy change for the system when 2.07 moles of N₂ (g) react at standard conditions. Substance So ASO = system NO(g) N₂ (9) O2(g) J/K J K. mol 210.8 191.6 205.1
I only want number 2 answered. The question is based on number one
The following gas-phase reaction takes place in a closed, constant-volume batch reactor at isothermal (constant temperature) conditions. 2CO+O2→2CO2 Initially, the reactor contains 0.564 kmol of CO, 1 kmol of O2, 1 kmol of CO2, and 0.5 kmol of N2 at a total pressure of 5 atm. At time t, the reactor pressure is 4.5 atm. Assuming ideal gas behavior, what is the extent of reaction (in kmol) at time t?
Solve the following questions related to fugacity of a liquid. Assume that liquid is incompressible and thus the = 1 molar volume of the liquid is constant. (You may assume that Psat is low enough that sat for all parts of this problem. You will also need to look up or calculate the molar volume of water.) You are given a container partially filled with water at 25°C. You then proceed to pump all of the air out of the container, leaving a pool of water at the bottom, and a vacuum (P=0) at the top (see first panel in figure below). You then turn off the pump and seal the container. You wait a short while and the water in the bottom starts to evaporate (see second panel) until it achieves phase equilibrium (see third panel). Assuming no change in temperature and no significant change in volume of the water, what is the pressure in the box? (Hint: you must balance fugacity between the liquid and vapor phases. You may also assume the vapor phase is an ideal gas, and the liquid is an ideal…
Consider the reaction: 2H₂O(1)→ 2H₂(g) + O2(g) Using standard absolute entropies at 298 K, calculate the entropy change for the system when 2.26 moles of H₂O(1) react at standard conditions. AS⁰⁰ Substance So system H₂(g) 02 (9) H₂O(1) J K mol 130.7 205.1 69.9 J/K
P.9 Assume that a sealed vessel at constant pressure of 1 bar initially contains 2.00 mol of NO₂(g). The system is allowed to equilibrate with respect to the reaction 2 NO₂(g) N₂O4(g). The number of moles of NO₂(g) and N₂O4(g) at equilibrium is 2.00 - 2 and , respectively, where is the extent of reaction. a. Derive an expression for the entropy of mixing as a func- tion of . b. Graphically determine the value of ₹ for which AS mixing has its maximum value. c. Write an expression for Gpure as a function of §. Use Equation 104 to obtain values of Gm for NO2 and N₂O4. d. Plot Gmixture = Gpure + AGmixing as a function of for ₹ T = 298 K and graphically determine the value of & for which Gmixture has its minimum value. Is this value the same as for part (b)?

Recommended textbooks for you

Introduction to Chemical Engineering Thermodynami…

Chemical Engineering

ISBN:

9781259696527

Author:

J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Publisher:

McGraw-Hill Education

Elementary Principles of Chemical Processes, Bind…

Chemical Engineering

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

Elements of Chemical Reaction Engineering (5th Ed…

Chemical Engineering

ISBN:

9780133887518

Author:

H. Scott Fogler

Publisher:

Prentice Hall

Introduction to Chemical Engineering Thermodynami…

Chemical Engineering

ISBN:

9781259696527

Author:

J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Publisher:

McGraw-Hill Education

Elementary Principles of Chemical Processes, Bind…

Chemical Engineering

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

Elements of Chemical Reaction Engineering (5th Ed…

Chemical Engineering

ISBN:

9780133887518

Author:

H. Scott Fogler

Publisher:

Prentice Hall

Process Dynamics and Control, 4e

Chemical Engineering

ISBN:

9781119285915

Author:

Seborg

Publisher:

WILEY

Industrial Plastics: Theory and Applications

Chemical Engineering

ISBN:

9781285061238

Author:

Lokensgard, Erik

Publisher:

Delmar Cengage Learning

Unit Operations of Chemical Engineering

Chemical Engineering

ISBN:

9780072848236

Author:

Warren McCabe, Julian C. Smith, Peter Harriott

Publisher:

McGraw-Hill Companies, The

SEE MORE TEXTBOOKS

QUESTION 9 Regarding the following reaction at constant temperature, calculate the ratio of Kx at total pressure of 5.0 bar to that at 1.5 bar. Please enter your answer with 1 decimal. For example, 0.567 is written as 0.6. H₂CO (g) = CO (g) + H₂ (g).