== Q5.60 Homework Unanswered Consider the decomposition reaction of ammonia at 723 K: 2 NH3(g) → N₂(g) + 3 H₂(g) AH = +92.6 kJmol-1 What is the corresponding change in internal energy (AU) for this reaction? Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5E5 for 2.5 x 105) Type your numeric answer and submit Unanswered 4 attempts left Submit

== Q5.60 Homework Unanswered Consider the decomposition reaction of ammonia at 723 K: 2 NH3(g) → N₂(g) + 3 H₂(g) AH = +92.6 kJmol-1 What is the corresponding change in internal energy (AU) for this reaction? Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5E5 for 2.5 x 105) Type your numeric answer and submit Unanswered 4 attempts left Submit

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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When a chemist burns ammonia according to the reaction below she finds that the reaction releases heat. (It is exothermic.) 4NH3(g) + 3O2(g) 2N2(g) + 6H2O(g) The enthalpy of the reaction DH = -1267 kJ. What is the enthalpy change (in kJ) when 3 grams of ammonia are burned?
BE’s are: C=O 799, C–H 413, O–H 467, O–O 498, H–H 432 kJ/mol CO2(g) + 4H2(g) → CH4(g) + 2H2O(g) ΔHrxn° = ___ kJ (from ΔHf°s) ΔHrxn°(BE) = ___ kJ (from BEs) = (2x799+432-4x413-4x467) CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) ΔHrxn° = ___ kJ (from ΔHf°s) ΔHrxn°(BE) = ___ kJ (from BEs) ...Calculate ΔHrxn°s from both!
Please assist me with my practice question. The combustion of butane is shown by the following equation: 2C4H10 (l) + 13O2 (g) → 8CO2 (g) + 10H2O(g) Use the following data and the summing method to find the heat of reaction for the above equation. Note: Show all calculations, follow the rules of significant figures, and box your final answer. C(s) + O2 (g) → CO2 (g) + 393 kJ H2 (g) + ½O2 (g) → H2O(g) + 242 kJ 4C(s) + 5H2 (g) → C4H10 (g) + 125 kJ
When ammonia is oxidized it produces nitrogen monoxide and heat: 4NH3(g)+ 5O2(g)--> 4NO(g) +6H2O(g) "Triangle symbol"H degrees= -906kJ (a) Is the reaction endothermic or exothermic? Explain your answer. (b) If the reaction is carried out in a bomb calorimeter, will the temperature of the calorimeter increase or decrease? Explain your answer. (c) Is the internal energy of the products or reactants higher? Explain your answer.
What is the AH of the following hypothetical reaction? 2A(s) + B2(g) → 2AB(g) Given: A(s) + B2(g) → AB2(g) 2AB(g) + B2(g) –→ 2AB2(g) AH = -187.5 kJ AH = -771.5 kJ Enter your answer in decimal notation with four significant fiqures.
Q 1 please
Use the References to access important values if needed for this question. The following thermochemical equation is for the reaction of methane(g) with water(g) to form hydrogen(g) and carbon monoxide(g). CH4(g) + H20(g)3H2(g) + CO(g) →3H2(g) + CO(g) AH = 206 kJ When 6.16 grams of methane(g) react with excess water(g), kJ of energy are Hint: An amount of energy is expressed as a positive number. The sign of AH in the thermochemical equation indicates whether the energy is absorbed or evolved.
33 of 35 > Macmillan Learning When methanol, CH3OH, is burned in the presence of oxygen gas, O₂, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation CH₂OH(g) + O₂(g) → CO₂(g) + 2 H₂O(1) ΔΗ = −764 kJ How much methanol, in grams, must be burned to produce 601 kJ of heat? mass:
TUMU Consider these reactions: Reaction 1: H₂(g) + Cl₂(g) → 2HCl(g) AH = -184.6 kJ Reaction 2: 20F 2(g) → O₂(g) + 2 F₂ (g) Reaction 3: N₂(g) +202(g) →→→ 2NO₂(g) Use Reaction 1. Answer: AH = -49.4 kJ Determine the mass, in grams, of chlorine gas consumed (with excess H₂) when 1,152.0 kJ of energy is released from the system. Round to the nearest whole number. g AH = +66.4 kJ