6. The oxidation of methylhydrazine, N,H,CH,(1),by dinitrogen tetroxide, N,O,(1), was used forpropulsion in the Space Shuttle orbiter. Thisreaction is represented by the equation4 N,H,CH;(1) + 5 N,0,(1) →12 H,O(g) + 9 N,(g) + 4 CO,(g)The enthalpy of formation for liquidmethylhydrazine is +53 kJ/mol and the enthalpy offormation for liquid dinitrogen tetroxide is-20 kJ/mol. Calculate AH° for this reaction. KU A

Answered: Image /qna-images/answer/e8130aaa-49c6-44d9-b88c-eb52f3ca134c.jpg

6. The oxidation of methylhydrazine, N,H,CH,(), by dinitrogen tetroxide, N,0,(1), was used for propulsion in the Space Shuttle orbiter. This reaction is represented by the equation 4 N,H,CH,() + 5 N,0,(1) → 12 H,O(g) + 9 N,(g) + 4 CO,(g) The enthalpy of formation for liquid methylhydrazine is +53 kJ/mol and the enthalpy of formation for liquid dinitrogen tetroxide is -20 kJ/mol. Calculate AH° for this reaction. KU |

6. The oxidation of methylhydrazine, N,H,CH,(), by dinitrogen tetroxide, N,0,(1), was used for propulsion in the Space Shuttle orbiter. This reaction is represented by the equation 4 N,H,CH,() + 5 N,0,(1) → 12 H,O(g) + 9 N,(g) + 4 CO,(g) The enthalpy of formation for liquid methylhydrazine is +53 kJ/mol and the enthalpy of formation for liquid dinitrogen tetroxide is -20 kJ/mol. Calculate AH° for this reaction. KU |

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...

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Zinc is commonly found in nature in the form of the min- eral sphalerite (ZnS). A step in the smelting of zinc is the roasting of sphalerite with oxygen to produce zinc oxide: 2 ZnS(s) + 3 O2(g)→ 2 ZnO(s) + 2 SO2(g) (a) Calculate the standard enthalpy change AH° for this reaction, using data from Appendix D. (b) Calculate the heat absorbed when 3.00 metric tons (1 metric ton = 103 kg) of sphalerite is roasted under constant-pressure conditions.
Please answer both questions as they are calculated together but just a heads up they are different questions. Thank you for helping me
A scientist measures the standard enthalpy change for the following reaction to be 6.7 kJ : CO(g) + H,O(1)–CO;{g) + H2(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of CO(g) is kJ/mol.
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Given the following reactions and their enthalpies: AH(kJ/mol) H;(g) 2H(g) 20(g) +436 O:(g) +495 H,(g) + 0,(g) → H,O(g) -242 (a) Devise a way to calculate AH for the reaction H,O(g) - 2H(g) + O(g) (b) From this, estimate the H-O bond energy.
Hydrazine, N3H4, is a colorless liquid used as a rocket fuel. What is the enthalpy change for the process in which hydrazine is formed from its elements? N3(9) + 2H2 (9) + N2H4 (1) Use the following reactions and enthalpy changes: N2H, (1) + O2 (9) + N2(9) + 2H, 0(1); AH = -622.2 kJ H2 (9) +O2(g) H20(1); AH = -285.8 kJ ΔΗ- k)
What is the standard enthalpy of formation of carbon dioxide?
The compound WO3(s) is utilized in the refining process of tungsten from its mineral ore. Tungsten can be produced as follows: Reaction 1: WO3(s) + 3H2(g) → W(s) + 3H2O(g) a) From the following data calculate the enthalpy of the above reaction Reaction 2: 2W(s) + 3O2(g) → 2WO3(s) ΔH = –1685.4 kJ Reaction 3: 2H2(g) + O2(g) → 2H2O(g) ΔH = –477.84 kJb) Estimate the change of internal energy for Reaction 1. c) Is Reaction 1 exothermic or endothermic?
Ethylene glycol, HOCH2CH2OH, is used as antifreeze. It is produced from ethylene oxide, C2 H40, by the reaction C2 H4O(g) + H,0(1) HOCH, CH,OH(!) Use Hess's law to obtain the enthalpy change for this reaction from the following enthalpy changes: 2C, HO(g) + 502(9) → 4CO2 (9) + 4H,0(1) AH =-2612.2 kJ HOCH, CH, OH(1) + O2 (9) → 2002 (9) + 3H,0(1) AH=-1189.8 kJ Enthalpy change = kJ %3D
Find the enthalpy of reaction for the equation: H2SO4laq) + 2NAOH(aq)-Na,SO,(aq) + 2H20(), AH=? Using the following equations whose enthalpy is known (please round your answer to the tenths place): H2(g) + S(s) + 202(g) – H2SO,(aq), AH= -907.5 kJ Na(s)+ ½H2(g) + ½O2{g) – NaOH(aq), AH= -469.6 kJ 2Na(s) + S(s) + 20,(g) – Na,SOal(aq). AH= -1387.1 kJ H2(8) + ½O2(g) – H2O(1). AH= -285.8 kJ AH= kJ.
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(b) An aqueous solution of acetic acid can be prepared by the reaction of ethanol with oxygen : CH3CH2OH (1) + O2 (g) –→ CH3COOH (1) + H2O (1) Write thermochemical equations for enthalpy of formation of the given compounds and calculate AH for the reaction, given the following data. Enthalpy of formation, AHf (kJmol") -277.8 Compound CH;CH2OH (1) CH3COOH (I) H2O (1) -485.0 -286.0