The chemical equation that represents the combustion of methane is CH4(9) +20₂(9) - CO₂(g) + 2H₂O(g) An enthalpy diagram that represents the combustion of methane Ep (kJ) Ep (ku) • • • + reactant molecules • The difference between the enthalpy of the products and the enthalpy of the reactants is the "enthalpy change" and is represented by number • 239 154 • 37.0 endothermic -312 A bonds breaking 2648 Using the diagram above, calculate the following values Record your numerical answer; do not include units • separated atoms Energy Pathway Diagram Reaction Coordinate Reaction Coordinate 3450 bonds making exothermic -(~) АН product molecules kJ Activation energy for the forward, catalyzed reaction. KJ Enthalpy of reaction for the reverse catalyzed reaction. KJ Activation energy for the reverse, uncatalyzed reaction. kJ Enthalpy of reaction for the forward, uncatalyzed reaction. kJ Activation energy for the forward, uncatalyzed reaction. kJ Enthalpy of reaction for the reverse uncatalyzed reaction. kJ Activation energy for the reverse, catalyzed reaction. kJ Enthalpy of reaction for the forward, catalyzed reaction.

The chemical equation that represents the combustion of methane is CH4(9) +20₂(9) - CO₂(g) + 2H₂O(g) An enthalpy diagram that represents the combustion of methane Ep (kJ) Ep (ku) • • • + reactant molecules • The difference between the enthalpy of the products and the enthalpy of the reactants is the "enthalpy change" and is represented by number • 239 154 • 37.0 endothermic -312 A bonds breaking 2648 Using the diagram above, calculate the following values Record your numerical answer; do not include units • separated atoms Energy Pathway Diagram Reaction Coordinate Reaction Coordinate 3450 bonds making exothermic -(~) АН product molecules kJ Activation energy for the forward, catalyzed reaction. KJ Enthalpy of reaction for the reverse catalyzed reaction. KJ Activation energy for the reverse, uncatalyzed reaction. kJ Enthalpy of reaction for the forward, uncatalyzed reaction. kJ Activation energy for the forward, uncatalyzed reaction. kJ Enthalpy of reaction for the reverse uncatalyzed reaction. kJ Activation energy for the reverse, catalyzed reaction. kJ Enthalpy of reaction for the forward, catalyzed reaction.

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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Carbon disulfide is a colorless liquid. When pure, it is nearly odorless, but the commercial product smells vile. Carbon disulfide is used in the manufacture of rayon and cellophane. The liquid burns as follows: CS2 (1) +302 (9) → CO2(9) + 2SO2 (g) Calculate the standard enthalpy change for this reaction using standard enthalpies of formation. AH;(CS2 (1)) = 89.70 kJ/mol AH;(02(9)) = 0 kJ/mol %3D AH;(CO2 (g)) =-393.52 kJ/mol AH;(SO2 (g)) =-296.8 kJ/mol %3D Standard enthalpy change = kJ
[References] Carbon disulfide is a colorless liquid. When pure, it is nearly odorless, but the commercial product smells vile. Carbon disulfide is used in the manufacture of rayon and cellophane. The liquid burns as follows: CS2 (1) +302(9) CO2(g) + 2S02(g) Calculate the standard enthalpy change for this reaction using standard enthalpies of formation. AH;(CS2(1)) = 89.70 kJ/mol AH;(02(9)) = 0 kJ/mol AH;(CO2(9)) = -393.52 kJ/mol AH;(SO2 (9)) = -296.8 kJ/mol Standard enthalpy change = kJ Submit Answer Try Another Version 5 item attempts remaining Previous Next Email Instructor Save and Exit Cengage Lening | Cengage Technical Support 10:35 PM e to search 2 48°F Cloudy 12/6/2021
Tetrachloromethane, CCl4, is formed from methane and chlorine in the following reaction: CH4 (g) + 4 Cl₂ (g) → 4 HCl(g) + CCl4 (g) = Calculate A₁H, the enthalpy change for this reaction, using the enthalpies of formation of CO₂ (g), H₂O(l), and CCl4 (g), (▲ƒ H° = enthalpy changes for the following reactions: CH4 (g) + 2 O2(g) → 2 H₂O(l) + CO₂(g) ΔΗ° :-890.4 kJ/mol-rxn 2 HCl(g) → H₂(g) + Cl₂ (g) ΔΗ° +184.6 kJ/mol-rxn = ΔΗ° = Compound AfH (kJ/mol) H₂O(g) CO₂(g) -285.8 -393.5 kJ/mol-rxn - 95.98 kJ/mol), and the
The standard heat of formation, AH, is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have AH = 0. Heat of formation values can be used to calculate the enthalpy change of any reaction. Part A For which of the following reactions is AH equal to AH of the product(s)?You do not need to look up any values to answer this question !3! Check all that apply. Consider, for example, the reaction > View Available Hint(s) 2NO(g) + O2(g) = 2NO2(g) with heat of formation values given by the following table: O 2Na(s) + Ch (x)-2NACI(s) O H,O, (g)→02(g) + H,O(g) AH (kJ/mol) Substance NO(g) - Na(s) +C½(1)¬NACI(s) 90.2 O2(g) O 2H,(g) + O2(g)--2H,O(g) NO2 (g) 33.2 O H2(g) + 0,(g)→H,O(g) Then the standard heat of reaction for the overall reaction is o Na(s) +Cl, (g)¬NACI(s) AH= AH; (products)- AH (reactants) 2(33.2) 12(90.2) + 0) Submit Previous Answers Request Answer 114 kJ P Pearson…
1. Calculate the enthalpy of reaction for the combustion of methane gas, CH4, to form CO,(g) + H,O(1).
4. Using ethanol as a fuel reduces greenhouse gas emissions by 40-50% when compared directly to gasoline. Calculate the enthalpy change for the combustion of ethanol, using the enthalpies of formation for C2H5OH), CO2(g), and H2Ou, located on the chart provided for the following reaction: C2H5OH(1) + 302(g) → 2CO2(g) + 3H2O1)
An intermediate step in the industrial production of nitric acid involves the reaction of ammonia with oxygen to form nitrogen monoxide and water. Given the following UNBALANCED reaction, calculate the enthalpy change for this reaction. *Include all necessary calculations and work required for obtaining the enthalpy of reaction. NH3 (g) + O2 (g) → NO (g) + H2O (g) ΔHrxn = ?
For which one of the following is the enthalpy of the reaction the same as the enthalpy of formation? A) H, (9) + F, (g) -2 HF (g) B) Ca (s) + ½ 0, (g) → CaO (s) C) 2 CH,OH (1) + 3 0, (g) → 2 CO, (g) + 4 H,O(g) D) Sro (s) + CO, (g) → → SrCO, (s) MacBook Air DI 80 888 F7 F5 F3 F4 F2 & #3 3 @ $ % 4 5 6 7 8 9 2 P W E R Y F J K. D C V B N
A scientist measures the standard enthalpy change for the following reaction to be -112.0 kJ : 2NO(g) + O2(g)–2NO2(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of NO2(g) is kJ/mol.
Determine the enthalpy of reaction: 2NH3+2CH4+302=2HCN+6H2O
The enthalpy of formation for H2O(g), CO2(g), and C2H5OH(l), in kJ/mol, are given as follows: DHfo[H2O(g)] = –241.8; DHfo[CO2(g)] = –393.5, and DHfo[C2H5OH(l)] = –277.6 How much heat is produced if 2.00 mole of ethanol (C2H5OH) is completely combusted according to the following equation? C2H5OH(l) + 3O2(g) --> 2CO2(g) + 3H2O(g); (A) 2470 kJ (B) 1230 kJ (C) 1790 kJ (D) 3580 kJ
Please answer both questions as they are calculated together but just a heads up they are different questions. Thank you for helping me