Calculate AHxn for the following reaction: 7C(s) + 8H₂(g) → C7H16 (1) Use the following reactions and given AH values: AH CH₁s (1)+1102(g) → 7CO2(g) +8H₂O(g), C(s) + O2(g) → CO₂(g), ΔΗ ΔΗ 2H₂(g) + O₂(g) → 2H₂O(g), AH Express your answer to four significant figures in kilojoules. ▸ View Available Hint(s) VE ΑΣΦ DMC) kJ -4464.3 kJ 393.5 kJ 483.5 kJ

Calculate AHxn for the following reaction: 7C(s) + 8H₂(g) → C7H16 (1) Use the following reactions and given AH values: AH CH₁s (1)+1102(g) → 7CO2(g) +8H₂O(g), C(s) + O2(g) → CO₂(g), ΔΗ ΔΗ 2H₂(g) + O₂(g) → 2H₂O(g), AH Express your answer to four significant figures in kilojoules. ▸ View Available Hint(s) VE ΑΣΦ DMC) kJ -4464.3 kJ 393.5 kJ 483.5 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...

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Given the reaction of 4 C (s) + 3 H2 (g) + O2 (g) → 2 C,H2 OH (1) AH = ΔΗ - 542 J What would the AH for 4 C2H2 OH (1) → 8 C (s) + 6 H2 (g) + 2 O2 (g) be? O-271 J 1084 J O -1084 J 271 J
18. (a) Molecule N₂H4 (1) + 2 H₂O2 (1) → N2(g) + 4 H₂O (1) Complete the following table: Lewis Dot Structure (use dots or lines to show bonds) (b) (c) (d) N₂H4 H₂O2 N₂ H₂O Calculate the AH°rxn using average bond energies (Table 9.4 in textbook) Calculate the AH°rxn using the standard enthalpies of formation (Appendix 2 in textbook) Why are these two values slightly different?
Combustion reactions involve reacting a substance with oxygen. When compounds containing carbon and hydrogen are combusted, carbon dioxide and water are the products. Using the enthalpies of combustion for C₂H₂ (-1300. kJ/mol), C₂H6 (-1560. kJ/mol), and H₂ (-286 kJ/mol), calculate AH for the reaction C₂H₂(g) + 2H₂(g) → C₂H6 (9) ΔΗ - Submit Answer Try Another Version Titem attempt remaining Cengage Learning Cengage Technical Support Previous Next> Email Instructor Save and Exit
Use the chemical equation below to complete the conversion factor: 6H₂O (1) + 6CO2 (g) → C6H12O6 (s) + 602 (9) 7 mol C HO ? kJ heat mol C6H12O6 kJ heat of reaction = +2803 kJ
1. Draw Lewis structures for ozone and for dioxygen. Using the data given below, qualitatively compare the bond enthalpies, bond orders, and bond lengths of these two compounds. O₂ (g) 20 (g) AH" = +498 kJ O(g) + O₂(g) →O, (g) AH-105 kJ
The bombardier beetle uses an explosive discharge as a defensive measure. The chemical reaction involved is the oxidation of hydroquinone by hydrogen peroxide to produce quinone and water: CоHа (ОН)2 (ад) + H202(аg) — СөН, О2(ад) + 2H2О() Calculate AH for this reaction from the following data: CвНа (ОН)2(аq) — СеH4О2(ад) + H2(9) ДН — 177.4 kJ H2 (g) + O2 (g) → H2O2(ag) AH = -191.2 kJ H2 (g) + 02 (g) → H2O(g) AH = -241.8 kJ H2O(g) → H20(1) AH = -43.8 kJ ΔΗ kJ
Using the information below, calculate AH of NH3(g) + HCI(g) NH,CI(s). N, (8) + H, (8) NH,(g) AH = -46.19 kJ/mol > H, (g) + Cl,(8) → HCl(g) AH = -92.30 kJ/mol N, (8) + 2 H, (g) +Cl,(g) NH,Cl(s) AH = –314.4 kJ/mol • Your answer should have four significant figures. Provide your answer below: kJ/mol
Given the following reactions: Fe2O3(s) + 3 CO(g)→2 Fe(s) + 3 CO2(g); ΔH = −28.0kJ 3 Fe(s)+ 4 CO2(g) →4 CO(g) + Fe3O4(s); ΔH = +12.5 kJ the enthalpy of the reaction of Fe2O3 with CO 3 Fe2O3(s) + CO(g) → CO2(g) + 2 Fe3O4(s) is which of the following? -109 kJ -15.5 kJ +109 kJ -59.0 kJ
Given the following reactions Fe2O3 (s) + 3CO (s) → 2Fe (s) + 3CO2 (g) ΔH = –28.0 kJ mol–1 3Fe (s) + 4CO2(s) → 4CO (g) + Fe3O4(s) ΔH = +12.5 kJ mol–1 Determine the enthalpy of the following reaction in kJ mol–1 3Fe2O3 (s) + CO (g) → CO2 (g) + 2Fe3O4 (s) Select one: a. 40.5 b. +109 c. –109 d. –59.0 e. –15.5
The following table contains some standard enthalpies of formation, AH, at 298 K. Substance diamond graphite carbon tetrachloride carbon tetrachloride carbon tetrafluoride methane carbon monoxide carbon dioxide chlorine gas Cl₂ (g) hydrochloric acid fluorine gas hydrofluoric acid hydrogen oxygen water water hydrogen peroxide hydrogen peroxide ΔΗ (kJ/mol) 1.88 Formula C(s) C(s) 0 CCl4 (g) -106.7 CC14 (1) -139.3 CF4 (g) CH4 (g) -74.8 CO(g) -110.5 -679.9 CO₂(g) -393.5 0 HCl(g) -92.30 F2 (g) 0 HF (g) -268.61 H₂(g) 0 O2 (g) 0 H₂O(g) -241.82 H₂O(1) -285.83 H₂O2(g) -136.10 H₂O2 (1) -187.8
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.
Consider the following chemical reaction: C3H8(g) + H2(g) to give C2H6(g) + CH4(g) ΔH° = ? Calculate the enthalpy change for the reaction above using Hess's law Thermochemical data: H2(g) + 1\2O2(g) to give H2O(l) ΔH° =-285.8 kJ ΔH° combustion for CH4(g) ΔH° =-890.0 kJ/mol CO2 giving C(s, graphite) + O2(g) ΔH°= +393.5 kJ ΔH° combustion for C2H6(g) ΔH° =-1560.0 kJ/mol ΔH°f for C3H8(g) ΔH° =-103.8 kJ/mol