Hydrazine and 1,1-dimethylhydrazine both react spontaneously with O2 and can be used as rocket fuels. N2H4 () + O2 (g) N2(g) + 2 H2O(g) N2H2 (CH3 )2 (4) + 4 02 (g) 2 CO2 (g) +4 H2O(g) + N2 (g) The molar enthalpy of formation of N,H4 (e) is +50.6 kJ/mol, and that of N3H2 (CH3)2 () is +48.9 kJ/mol. Use these values, with other A,H values in the table below. Compound H2O(g) CO2 (8) A,H" (kJ/mol) -241.83 -393.509 Calculate the specific heat of the reaction hydrazine with oxygen. A,H - -16.7 V kJ/g hydrazine Correct To calculate molar enthalpy of the reaction, the sum of molar standard enthalpies of formation of reactants should be subtracted from molar standard enthalpies of formation of products: A,H (kJ/mol) = 2 mol x (-241.83 kJ/mol) - 1 mol x x 50.6 kJ/mol =-534.3 kJ/mol Convert the value from (kJ/mol) to (kJ/g): 1 mol (N, H4) 32.05 g (N,H4) A,H (kJ/g) = -534.3 kJ/mol x -16.67 kJ/g b Calculate specific heat of the reaction 1,1-dimethylhydrazine with oxygen. A,H -[ k//g 1,1-dimethylhydrazine Previous Next
Hydrazine and 1,1-dimethylhydrazine both react spontaneously with O2 and can be used as rocket fuels. N2H4 () + O2 (g) N2(g) + 2 H2O(g) N2H2 (CH3 )2 (4) + 4 02 (g) 2 CO2 (g) +4 H2O(g) + N2 (g) The molar enthalpy of formation of N,H4 (e) is +50.6 kJ/mol, and that of N3H2 (CH3)2 () is +48.9 kJ/mol. Use these values, with other A,H values in the table below. Compound H2O(g) CO2 (8) A,H" (kJ/mol) -241.83 -393.509 Calculate the specific heat of the reaction hydrazine with oxygen. A,H - -16.7 V kJ/g hydrazine Correct To calculate molar enthalpy of the reaction, the sum of molar standard enthalpies of formation of reactants should be subtracted from molar standard enthalpies of formation of products: A,H (kJ/mol) = 2 mol x (-241.83 kJ/mol) - 1 mol x x 50.6 kJ/mol =-534.3 kJ/mol Convert the value from (kJ/mol) to (kJ/g): 1 mol (N, H4) 32.05 g (N,H4) A,H (kJ/g) = -534.3 kJ/mol x -16.67 kJ/g b Calculate specific heat of the reaction 1,1-dimethylhydrazine with oxygen. A,H -[ k//g 1,1-dimethylhydrazine Previous Next
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
please answer question B
the answer in a is for reference.
Calculate specific heat of the reaction 1,1-dimethylhydrazine with oxygen.
Transcribed Image Text:Hydrazine and 1,1-dimethylhydrazine both react spontaneously with O2 and can be used as rocket fuels.
N2H4 () + O2 (g) N2(g) + 2 H2O(g)
N2H2 (CH3 )2 (4) + 4 02 (g) 2 CO2 (g) +4 H2O(g) + N2 (g)
The molar enthalpy of formation of N,H4 (e) is +50.6 kJ/mol, and that of N3H2 (CH3)2 () is +48.9 kJ/mol. Use
these values, with other A,H values in the table below.
Compound
H2O(g)
CO2 (8)
A,H" (kJ/mol)
-241.83
-393.509
Calculate the specific heat of the reaction hydrazine with oxygen.
A,H - -16.7
V kJ/g hydrazine
Correct
To calculate molar enthalpy of the reaction, the sum of molar standard enthalpies of formation of reactants
should be subtracted from molar standard enthalpies of formation of products:
A,H (kJ/mol) = 2 mol x (-241.83 kJ/mol) - 1 mol x
x 50.6 kJ/mol =-534.3 kJ/mol
Convert the value from (kJ/mol) to (kJ/g):
1 mol (N, H4)
32.05 g (N,H4)
A,H (kJ/g) = -534.3 kJ/mol x
-16.67 kJ/g
b Calculate specific heat of the reaction 1,1-dimethylhydrazine with oxygen.
A,H -[
k//g 1,1-dimethylhydrazine
Previous
Next
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 1 images
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