Compounded with carbon. Carbon double bonds, such as ethylone O₂ Hy add hydrogen in a reaction called hydrogenation. Calculate the enthalpy, Change for this reaction, lesing the Combussion data and Helis low. C₂ Hut На -C2₂H6 (3C2H4 + 902 →600₂ + 6H₂0 DH = 1401 kJ (ii) 2 C₂H6+ 7 Q₂ + 4CO₂ + 6H₂ODH = 3 sookJ (11) 24₂ +1 0₂ > 21120 DH=572KJ

Compounded with carbon. Carbon double bonds, such as ethylone O₂ Hy add hydrogen in a reaction called hydrogenation. Calculate the enthalpy, Change for this reaction, lesing the Combussion data and Helis low. C₂ Hut На -C2₂H6 (3C2H4 + 902 →600₂ + 6H₂0 DH = 1401 kJ (ii) 2 C₂H6+ 7 Q₂ + 4CO₂ + 6H₂ODH = 3 sookJ (11) 24₂ +1 0₂ > 21120 DH=572KJ

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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Lauto.d21?ou=2194845&isprv3D&drc=0&qi=2824083&cfql=0&dnb=D0&f Calculate the standard enthalpy change for the reaction 2C8H18(1) + 17O2(g) → 16CO(g) + 18H20(1) Given: 2C3H18(1) + 2502(g) – 16CO2(g) + 18H20(1) AH° = -11020 kJ/mol 2C0(g) + O2(g) – 2CO2(g) AH° = -566 kJ/mol a) 10450 kJ/mol b) -6492 kJ/mol O c) 15550 kJ/mol d) 6492 kJ/mol e) -10450 kJ/mol
a) Using the balanced equation and the data in the table below, calculate the theoretical enthalpy of combustion. Note: you will need to include the enthalpy of vaporisation for the liquid components which are also given. CH3OH() +1.502(g) → CO2(g) + 2H2O (1) Average Bond Enthalpies (kJ mol‍¹) C-H C-C C-O O=O C=O O-H Enthalpy of Vaporisation (kJ mol-¹) Methanol Water 412 348 358 496 743 463 35 41
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Calculate the enthalpy of reaction
4.From these data: N2H4(l) + O2(g) à 2N2(g) + 2H2O(l) H= -622.2 kJ/mol H2(g) + ½O2 à H2O(l) H= -285.8 kJ/mol H2(g) + O2(g) à H2O2(l) H= -115 kJ/mol Find H for the reaction: N2H4(l) + 2H2O2(l) à 2N2(g) + 4H2O(l)
Given the enthalpies for the following reactions: 2 Fe (s) + 3/2 O₂(g) → Fe2O3 (s)Math output error AH₂ ΔΗ, CO (g) + 1/2 O₂ (g) → CO₂ (g) CO2 (g) ΔΗ = -248.7 kJ rxn rxn = 1,091.6 kJ Calculate the enthalpy change (AHrxn) for the following reaction: Fe2O3 (s) + 3 CO (g) → 2 Fe (s) + 3 CO₂ (g)
b) Construct an enthalpy cycle and calculate the enthalpy of combustion in each case using the above data. 3. Given the following data: AH(CH4) = -74.8 kJmol-¹, AH(CH3CI) = -134.5 kJmol-¹, AH (HCI) = -92.3 kJmol-¹; Construct an enthalpy cycle and calculate H for the reaction CH4(g) + Cl2(g) CH3CI(g) + HCl(g) 4. Given the data: 4NH3(g) + 302(g) 0 2N2(g) + 6H2O(1), AH = -1530kJmol-1 H2(g) + 1/2O2(g) □ H₂O(1), AH = -288 kJmol-¹ Construct an enthalpy cycle and calculate the enthalpy of formation of ammonia.
Consider the following reaction: CH4 (9) + 20, (g) → CO2(g) + 2H,0(1) AH=-891 kJ a. Calculate the enthalpy change if 2.59 g methane is burned in excess oxygen. Enthalpy change = kJ b. Calculate the enthalpy change if 3.04 × 10° L methane gas at 737 torr and 25°C is burned in excess oxygen. Enthalpy change = kJ
Give only typing answer with explanation and conclusion Given that N2 (g) + 3 H2 (g) → 2 NH3 (g) ΔH° = -92 kJ H2 (g) + Cl2 (g) → 2 HCl (g) ΔH° = -185 kJ N2 (g) + 4 H2 (g) + Cl2 (g) → 2 NH4Cl (g) ΔH° = -629 kJ determine the standard enthalpy change for the reaction shown below: NH3 (g) + HCl (g) → NH4Cl (s)
Calculate AH, (kJ/mol), enthalpy of formation, for the hypothetical CaF(s) given: AHjattice = -795 kJ/mol AHsub(Ca) = +178 kJ/mol AHje1 (Ca) = +590 kJ/mol %3D AHje2 (Ca) = +1250 kJ/mol AH(F2) = +158 kJ/mol AHea(F) = -328 kJ/mol 1053 O -974 O 874 O 974 O 1053
4NH3(g) + 3O2(g) → 2N2(g) + 6H2O(l), ΔH = -1530kJmol-1 (1) H2(g) + 1/2O2(g) → H2O(l), ΔH = -288 kJmol-1 (2) Construct an enthalpy cycle and calculate the enthalpy of formation of ammonia.