Homework Help is Here – Start Your Trial Now!
Science
Chemistry
Methylhydrazine Chemical Formula CH,N2 Molar Mass 46.07 g/mol Standard boiling point (T°%) AH°vap at Tºb 364 K 40.37 kJ/mol Cliquid at 298.15 K AH°rgas at 298.15 K Molar heat capacity (liquid) Density (liquid) S° (liquid) at 298.15 K ΔΗ, 54.14 kJ/mol 94.50 kJ/mol 134.93 J/mol-K 0.878 g/cm³ 165.94 J/mol K Other thermochemical data at 298.15 K, 1 atm AH°rof CO2«g) AH°rof H2O1) -393.51 kJ/mol -285.83 kJ/mol A. Estimate the standard enthalpy of combustion of methylhydrazine based on the given standard enthalpy of formation values of reactants and products. B. Write the balanced thermochemical equation for the combustion of methylhydrazine. C. Calculate the heat evolved in the combustion of 25.00 liters of methylhydrazine at 298.15 K in air (external pressure of 760 mmHg).

Methylhydrazine Chemical Formula CH,N2 Molar Mass 46.07 g/mol Standard boiling point (T°%) AH°vap at Tºb 364 K 40.37 kJ/mol Cliquid at 298.15 K AH°rgas at 298.15 K Molar heat capacity (liquid) Density (liquid) S° (liquid) at 298.15 K ΔΗ, 54.14 kJ/mol 94.50 kJ/mol 134.93 J/mol-K 0.878 g/cm³ 165.94 J/mol K Other thermochemical data at 298.15 K, 1 atm AH°rof CO2«g) AH°rof H2O1) -393.51 kJ/mol -285.83 kJ/mol A. Estimate the standard enthalpy of combustion of methylhydrazine based on the given standard enthalpy of formation values of reactants and products. B. Write the balanced thermochemical equation for the combustion of methylhydrazine. C. Calculate the heat evolved in the combustion of 25.00 liters of methylhydrazine at 298.15 K in air (external pressure of 760 mmHg).

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

need some help in letters D and E

Methylhydrazine Chemical Formula CH,N2 Molar Mass 46.07 g/mol Standard boiling point (T°b) AH°vap at T°b AH°rliquid at 298.15 K AH°rgas at 298.15 K Molar heat capacity (liquid) Density (liquid) S° (liquid) at 298.15 K 364 K 40.37 kJ/mol 54.14 kJ/mol 94.50 kJ/mol 134.93 J/mol-K 0.878 g/cm³ 165.94 J/mol K Other thermochemical data at 298.15 K, 1 atm AH°rof CO2(g) -393.51 kJ/mol AH°rof H2Ot1) -285.83 kJ/mol A. Estimate the standard enthalpy of combustion of methylhydrazine based on the given standard enthalpy of formation values of reactants and products. B. Write the balanced thermochemical equation for the combustion of methylhydrazine. C. Calculate the heat evolved in the combustion of 25.00 liters of methylhydrazine at 298.15 K in air (external pressure of 760 mmHg). : 2/2 D. Calculate the approximate work involved in the combustion in air (external pressure of 1.00 atm) of 25.00 liters of methylhydrazine at 298.15 K. What assumption did you make for this calculation. E. Calculate the total energy (AU in kJ) involved when 15.0 moles of methylhydrazine are heated from 325 K to its boiling point (T°%) at 1.00 atm. Assume that the volume of methylhydrazine does not change significantly from 325 K to its T°p.
Transcribed Image Text:Methylhydrazine Chemical Formula CH,N2 Molar Mass 46.07 g/mol Standard boiling point (T°b) AH°vap at T°b AH°rliquid at 298.15 K AH°rgas at 298.15 K Molar heat capacity (liquid) Density (liquid) S° (liquid) at 298.15 K 364 K 40.37 kJ/mol 54.14 kJ/mol 94.50 kJ/mol 134.93 J/mol-K 0.878 g/cm³ 165.94 J/mol K Other thermochemical data at 298.15 K, 1 atm AH°rof CO2(g) -393.51 kJ/mol AH°rof H2Ot1) -285.83 kJ/mol A. Estimate the standard enthalpy of combustion of methylhydrazine based on the given standard enthalpy of formation values of reactants and products. B. Write the balanced thermochemical equation for the combustion of methylhydrazine. C. Calculate the heat evolved in the combustion of 25.00 liters of methylhydrazine at 298.15 K in air (external pressure of 760 mmHg). : 2/2 D. Calculate the approximate work involved in the combustion in air (external pressure of 1.00 atm) of 25.00 liters of methylhydrazine at 298.15 K. What assumption did you make for this calculation. E. Calculate the total energy (AU in kJ) involved when 15.0 moles of methylhydrazine are heated from 325 K to its boiling point (T°%) at 1.00 atm. Assume that the volume of methylhydrazine does not change significantly from 325 K to its T°p.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps with 3 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Thermodynamic Aspects of Phase Transitions
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
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