Hydrazine is an inorganic compound with the chemical formula N2H4. The reaction of hydrazine with chlorine trifluoride has been used in experimental rocket motors in the reaction below: 3N2H4 (1) + 4CIF3 (g) > 3N2 (g) + 12HF + 2C12 (8) (g) Calculate enthalpy change for the reaction given the following: (1) 2CIF3 + 2NH3 → N2 + 6HF + Cl2 (2) N2H4 + O2 → N2 + 2H2O (3) 4NH3 + 302 → 2N2 + 6H2O AH°= -1196 kJ AH°= - 622 kJ AH° = - 1530 kJ

Hydrazine is an inorganic compound with the chemical formula N2H4. The reaction of hydrazine with chlorine trifluoride has been used in experimental rocket motors in the reaction below: 3N2H4 (1) + 4CIF3 (g) > 3N2 (g) + 12HF + 2C12 (8) (g) Calculate enthalpy change for the reaction given the following: (1) 2CIF3 + 2NH3 → N2 + 6HF + Cl2 (2) N2H4 + O2 → N2 + 2H2O (3) 4NH3 + 302 → 2N2 + 6H2O AH°= -1196 kJ AH°= - 622 kJ AH° = - 1530 kJ

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

Similar questions

Calculate the enthalpy change for the following reaction 2H2S (g) + SO2 (g) → 3S (s) + 2H2O (g) from the following equations: (1) H2O(g) → H2(g) + 1/2 O2(g) Ho = 241.8 kJ (2) H2S(g) → H2(g) + S(s) Ho = 20.6 kJ ( 3) S(s) + O2(g) → SO2(g) Ho = - 296.8 kJ
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.
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)
Hydrogen peroxide, H2O2, is a colorless liquid whose solutions are used as a bleach and an antiseptic. H2O2 can be prepared in a process whose overall change is H2 (9) +O2 (9) → H2O2 (1) Calculate the enthalpy change using the following data: 2H2O2 (1) → 2H2O(1) +O2 (g); AH=-196.0 kJ H2 (g) + O2(g)→ H20(1); AH -285.8 kJ AH kJ %3D
When 1.42 g of iron reacts with 1.80 g of chlorine, 3.22 g of iron(II) chloride (FeCl2, molar mass = 126.75 g/mol) and 6.8 kJ of heat is produced. What is the enthalpy change for the reaction when 1 mole of iron(II) chloride is produced? round to sig figs
Determine the enthalpy of the reaction: 3Fe,O; (s) + CO (g) → CO, (g) + 2Fe;O4 (s), given the following reactions. 38. Fe,O3 (s) + 3CO (g) → 2Fe (s) + 3CO, (g) AH= -28.0 kJ 3Fe (s) + 4CO2 (s) → 4CO (g) + Fe;O4 (s) AH =+12.5 kJ A) 40.5 +109 -59.0 -109
(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
Fluorine (F2), the most electronegative element reacts with water in a different way compared to other halogens do. With excess water, fluorine reacts with water to produce hydrofluoric acid and oxygen gas in the following reaction: 2F2(g) + 2H2O() →4HF (1) + O2(g) Calculate AHrxn for the process above from the following information: AH= +571.6 kJ (a) AH= +542.0 kJ (b) 2H₂O(1)→ 2H2(g) + O2(g) 2HF (g) → H2(g) + F2(g) Which equation(s) will you flip? O a. Only equation (b) O b. Only equation (a) O c. Both equations will be flipped. O d. No equations will be flipped.
Use standard enthalpies of formation to determine ΔHoreaction for the following reaction: 2N2H4(l) + N2O4(g) →3N2(g) + 4H2O(g)
6. Calculate the enthalpy change of the following reaction between nitrogen gas and oxygen gas, given thermochemical equations (1), (2), (3). 2N2(g) + 502(g) → 2N₂O(g) 2H2(g) + O2(g) → 2H₂O) N₂O + H₂O → 2HNO30) 0₂(g) + ₂H₂(g) → HNO 3 (1) + (1) (2) (3) 1/2N2(8) AH = -572 kJ AH = -77 kJ| AH-174 kJ