A mixture of ideal gases consists of 3 kg of nitrogen and 5 kg of carbon dioxide at a pressure of 3 bar and a temperature of 20°C. Find (i) the mole fraction of each constituent, (ii) the equivalent molecular weight of the mixture, (iii) the equivalent gas constant of the mixture, (iv) the partial pressures and partial volumes, (v) the volume and density of the mixture, and (vi) the c, and c of the mixture. If the mixture is heated at constant volume to 40°C, find the changes in internal energy, enthalpy and entropy of the mixture. Find the changes in internal energy, enthalpy and entropy of the mixture if the heating is done at constant pressure. Take y: for CO, = 1.286 and N, = 1.4.
A mixture of ideal gases consists of 3 kg of nitrogen and 5 kg of carbon dioxide at a pressure of 3 bar and a temperature of 20°C. Find (i) the mole fraction of each constituent, (ii) the equivalent molecular weight of the mixture, (iii) the equivalent gas constant of the mixture, (iv) the partial pressures and partial volumes, (v) the volume and density of the mixture, and (vi) the c, and c of the mixture. If the mixture is heated at constant volume to 40°C, find the changes in internal energy, enthalpy and entropy of the mixture. Find the changes in internal energy, enthalpy and entropy of the mixture if the heating is done at constant pressure. Take y: for CO, = 1.286 and N, = 1.4.
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...
Related questions
Question
Pls answer only the sub part (iv), (v) and (vi) thank u
![12. A mixture of ideal gases consists of 3 kg of nitrogen and 5 kg of carbon dioxide at a pressure of 3 bar and
a temperature of 20°C. Find (i) the mole fraction of each constituent, (ii) the equivalent molecular weight
of the mixture, (iii) the equivalent gas constant of the mixture, (iv) the partial pressures and partial
volumes, (v) the volume and density of the mixture, and (vi) the c, and c, of the mixture.
If the mixture is heated at constant volume to 40°C, find the changes in internal energy, enthalpy and
entropy of the mixture. Find the changes in internal energy, enthalpy and entropy of the mixture if the
heating is done at constant pressure.
Take y: for CO, = 1.286 and N2 = 1.4.
[Ans. (i) 0.485, 0.515 ; (ii) 36.25 kg/kg mole ; (iii) 0.229 kJ/kg K ;
(iv) 1.455 bar, 1.545 bar ; 0.87 m³, 0.923 m³ ; (v) 1.79 m³, 4.46 kg/m³ ;
(vi) 0.92 kJ/kg K, 0.69 kJ/kg K ; 110.4 kJ, 147.2 kJ, 0.368 kJ/kg K ; 0.49 kJ/kg K]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F54c634de-ead1-43a6-8db0-8fb273ab6e75%2F035220c9-87b6-4d6b-bf87-b935c99b38e4%2F4pduq2t_processed.jpeg&w=3840&q=75)
Transcribed Image Text:12. A mixture of ideal gases consists of 3 kg of nitrogen and 5 kg of carbon dioxide at a pressure of 3 bar and
a temperature of 20°C. Find (i) the mole fraction of each constituent, (ii) the equivalent molecular weight
of the mixture, (iii) the equivalent gas constant of the mixture, (iv) the partial pressures and partial
volumes, (v) the volume and density of the mixture, and (vi) the c, and c, of the mixture.
If the mixture is heated at constant volume to 40°C, find the changes in internal energy, enthalpy and
entropy of the mixture. Find the changes in internal energy, enthalpy and entropy of the mixture if the
heating is done at constant pressure.
Take y: for CO, = 1.286 and N2 = 1.4.
[Ans. (i) 0.485, 0.515 ; (ii) 36.25 kg/kg mole ; (iii) 0.229 kJ/kg K ;
(iv) 1.455 bar, 1.545 bar ; 0.87 m³, 0.923 m³ ; (v) 1.79 m³, 4.46 kg/m³ ;
(vi) 0.92 kJ/kg K, 0.69 kJ/kg K ; 110.4 kJ, 147.2 kJ, 0.368 kJ/kg K ; 0.49 kJ/kg K]
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 6 steps
Knowledge Booster
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.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY