Using any resources available to you (e.g., textbook, CRC Handbook, online sources), obtain and use standard heats of formation and Hess' Law to calculate the standard heat of reaction AH° for the decomposition of H₂O2. Show ALL your work below, starting with the balanced equation, and summarize your results in the table provided. NOTE: Do NOT simply look up the value of AH for this reaction and write it below - you NEED to use standard heat of formation, show your work, etc. Heat of Formation for H₂O₂(aq) (kJ/mol) Heat of Formation for H₂O(1) (kJ/mol) Heat of Formation for O₂(g) (kJ/mol) Calculated AHpn (J/mol)

Using any resources available to you (e.g., textbook, CRC Handbook, online sources), obtain and use standard heats of formation and Hess' Law to calculate the standard heat of reaction AH° for the decomposition of H₂O2. Show ALL your work below, starting with the balanced equation, and summarize your results in the table provided. NOTE: Do NOT simply look up the value of AH for this reaction and write it below - you NEED to use standard heat of formation, show your work, etc. Heat of Formation for H₂O₂(aq) (kJ/mol) Heat of Formation for H₂O(1) (kJ/mol) Heat of Formation for O₂(g) (kJ/mol) Calculated AHpn (J/mol)

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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Constants | Periodic Table The standard enthalpy of formation (AH;) is the enthalpy change that occurs when exactly 1 mol of a compound is formed from its constituent elements under standard conditions. The standard conditions are 1 atm pressure, a temperature of 25 °C, and all the species present at a concentration of 1 M.A"standard enthalpies of formation table" containing AH; values might Part A AN What is the balanced chemical equation for the reaction used to calculate AH; of BaCO3 (s)? If fractional coefficients are required, enter them as a fraction (1.e. 1/3). Indicate the physical states using the abbreviation (s)., (1), or (g) for solid, liquid, or gas, respectively without indicating allotropes. Use (aq) for aqueous solution. look something like this: Substance AH Express your answer as a chemical equation. H(g) 218 kJ/mol > View Available Hint(s) H2(g) O kJ/mol Ba(s) OkJ/mol ΑΣΦ Ba (aq) -538.4 kJ/mol C(g) 71 kJ/mol C(s) O kJ/mol DA chemical reaction does inot occur for this…
F When Fe₂O3(s) reacts with H₂(g) to form Fe(s) and H₂O(g), 98.8 kJ of energy are absorbed for each mole of Fe₂O3(s) that reacts. Write a balanced thermochemical equation for the reaction with an energy term in kj as part of the equation. Note that the answer box for the energy term is case sensitive. Use the SMALLEST INTEGER coefficients possible and put the energy term in the last box on the appropriate side of the equation. If a box is not needed, leave it blank. 20 Submit Answer 4 R F F4 V + % 5 [Review Topics] [References] Use the References to access important values if needed for this question. Retry Entire Group T G ♫ TV STA © B + MacBook Air FG 6 A Y H 7 more group attempts remaining & 7 N U J * 8 00 - M DII I K ( 9 V H s DD F9 O + O P F10 P A + command option Previous F11 { = Next> Save and Exit 40) F12 A delete S retur
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When N₂(g) reacts with H₂(g) to form NH3(g), 92.2 kJ of energy are evolved for each mole of N₂(g) that reacts. Write a balanced thermochemical equation for the reaction with an energy term in kJ as part of the equation. Note that the answer box for the energy term is case sensitive. Use the SMALLEST INTEGER coefficients possible and put the energy term (including the units) in the last box on the appropriate side of the equation. If a box is not needed, leave it blank. + + +
Q.30. Calculate the heat of combustion AH, , 298K of solid oxalic acid (C2H2O4, s) at 25 °C and atmospheric pressure, using the standard molar enthalpies of formation. 1) Write the equation of this reaction and calculate, using the data, its standard enthalpy at 298K. 2) Explain why the standard enthalpy of formation of gaseous oxygen is zero? (Explain in one sentence only) Given: Standard molar enthalpies of formation at 298.15K Substance and State A¢H® (kJ/mol) C2H2O4(s) -829.9 C2H2O4(g) -731.8 CO2(g) -393 CO2(aq) -413.26 H2O(g) -241.8 H2O(1) -285.2 O2(g)
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Using Hess’s Law, calculate for the change in enthalpy of the given reactions.
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Using the given molar enthalpies of formation, determine the change in enthalpy for the combustion of 1 mole of methanol. , AH°; CH3OH (4) =- 238.6 kJ/mol AH°; CO2 (g) = - 110.5 kJ/mol AH°; H2O (g) = – 241.8 kJ/mol 3 CH3OH (e) +02 (g) → CO2 (g) + 2H2O (g)
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2) Consider the situation: 2CH,O, + 30) 4H,0 + e) AH --1453.0 kJ 2 CO, ΔΗ, 2(8) Showing your work, how much heat would this represent for the combustion of 12.74 mol of liquid methanol (CH4O0)? Answer to 1 decimal place. [K3] the follouing processes: (2 marks each) [C4]