Calculate AH for the reaction CH₂(g) + 1/2O₂(g) → CO(g) + 2 H₂(g) given the following data: Equation CH4(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(g) CH₂(g) + CO₂(g) → 2 CO(g) + 2 H₂(g) CH4(g) + H2O(g) → CO(g) + 3 Hz(g) ΔΗ= Submit Show Hints Submit Answer kj Retry Entire Group ΔΗ (kJ) -802 247 206 9 more group attempts remaining

Calculate AH for the reaction CH₂(g) + 1/2O₂(g) → CO(g) + 2 H₂(g) given the following data: Equation CH4(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(g) CH₂(g) + CO₂(g) → 2 CO(g) + 2 H₂(g) CH4(g) + H2O(g) → CO(g) + 3 Hz(g) ΔΗ= Submit Show Hints Submit Answer kj Retry Entire Group ΔΗ (kJ) -802 247 206 9 more group attempts remaining

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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Use the bond energies in the table to estimate the enthalpy of reaction for the oxidation of hydrogen sulfide 2 H2S (g) + 3 O2 (g) → 2 SO2 (g) + 2 H2O (g) Bond H—S O=O S=O S—O O—H Energy (kJ/mol) 347 498 523 87 463
Given the following reactions, what is the overall enthalpy change for the following reaction? N H 3 ( g ) + H C l ( g ) ⟶ N H 4 C l ( s ) Reaction ΔHo (kJ) N 2 ( g ) + 3 H 2 ( g ) ⟶ 2 N H 3 ( g ) -92 H 2 ( g ) + C l 2 ( g ) ⟶ 2 H C l ( g ) -185 N 2 ( g ) + 4 H 2 ( g ) + C l 2 ( g ) ⟶ 2 N H 4 C l ( s ) -629
Use the molar bond enthalpy data in the table to estimate the value of AH rxn for the equation CC1₂(g) + 2 F₂ (g) → CF₂(g) + 2Cl₂ (g) The bonding in the molecules is shown. +o+ AH rxn = F-F F-F F + + CI-CI CI-CI Average molar bond enthalpies (H bond) Bond C=N N-H N-N N=N N=N F-F Cl-Cl Br-Br H-H H-F H-Cl H-Br H-S S-S Bond O-H O-O C-O 0=0 C=O C-C C=C C=C C-H C-F C-Cl C-Br C-N C=N kJ.mol-¹ 464 142 351 502 730 347 615 811 414 439 331 276 293 615 kJ∙·mol¯¹ 890 390 159 418 945 155 243 192 435 565 431 368 364 225 kJ.mol-¹
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Use average bond energies to estimate the energy released when 70.0 g CH4 undergoes complete combustion: CH₂(g) +20₂(g) → CO₂(g) + 2H₂O(g) kJ 4
Use the indicated average bond enthalpies to estimate the change in enthalpy, ΔHo, for the reaction between methane and iodine to produce iodomethane and hydrogen iodide: CH4(g) + I2(g) → CH3I(g) + HI(g) ΔHo = ? It may be helpful to draw the Lewis electron dot structure for each reactant and product; all reactants and products have single bonds. average bond enthalpies (kJ) C - H 413 , C - I 240 , H - I 299 , I - I 151 Express your answer in units of kilojoules, but do not include the units on your submitted answer.
Part A Calculate the enthalpy of the reaction 2NO(9) + 02(9)→2NO2(g) given the following reactions and enthalpies of formation: A N2(g) + O2(9)→NO2(g), AfH = 33.2 kJ mol 1 B. N2 (9) + ¿O2(g)→NO(g), A;H = 90.2 kJ mol-1 Express your answer with the appropriate units. • View Available Hint(s) HA ? AfH° = Value Units
Using the equations 2 Fe (s) + 3 CI, (g) → 2 FeCl, (s) AH° = -800.0 kJ/mol Si(s) + 2 CI, (g) → SICI, (s) AH° = -640.1 kJ/mol %3D 4 Determine the enthalpy (in kJ/mol) for the reaction 3 SICI, (s) + 4 Fe (s) → 4 FeCl, (s) + 3 Si (s) kJ/mol
Calculate AH for the following reaction, given the data in the table below: H2SO4() → So:(g) + H2O(g) AH = ??? kJ/mol H2S(g) +202(g)→ H2SO4(1) AH = -749.7 kJ H,S(g) + 202(g) → SO3(g) + H2O(1) AH = -355.0 kJ H20(1) H20(g) AH = +53.95 kJ
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
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
Determine the enthalpy of reaction for the following: H2(g) + ¹/2O2(g) → H₂O(g)