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<> LTI Launch

Posted: Wed Jul 06, 2022 10:47 am

by answerhappygod

Lti Launch Homework Ch 9 Thermodynamics Adaptive Follow Up Exercise 9 90 Enhanced With Expanded Hints Missed Thi 1 (104.07 KiB) Viewed 20 times

<> LTI Launch <Homework Ch 9-Thermodynamics Adaptive Follow-Up Exercise 9.90 - Enhanced - with Expanded Hints MISSED THIS? Watch KCV 9.10, IWE 9.12; Read Section 9.10. You can click on the Review link to access the section in your e Text. The explosive nitroglycerin (C3H5N3O₂) decomposes rapidly upon ignition or sudden impact according to the following balanced equation: session.masteringchemistry.com M MasteringChemistry: Homework Ch 9-Thermodynamics Adaptive Fo... 4C3H5N3O9 (1)→→ 12CO2(g) + 10H₂O(g) + 6N2(g) + O₂(g) A Hin=-5678 kJ The heats of formation for carbon dioxide and water are AH (CO₂) = -393.5 kJ/mol and AH (H₂O) = -241.8 kJ/mol, respectively. Part A Calculate the standard enthalpy of formation (AH₂) for nitroglycerin. Express your answer in kilojoules per mole to four significant figures. ► View Available Hint(s) AH;= Submit ΫΠ ΑΣΦ - 365 Previous Answers C C The explosive nitroglycerin (C3H5N309) decomposes... | answers.com 1 +88 kJ/mol < Item 8 > Review | Constants | Periodic Table X Incorrect; Try Again; 4 attempts remaining The chemical equation for the decomposition of nitroglycerin needs to be reversed and normalized for 1 mol of C3H5N3O9: 3CO₂(g) + 2.5H₂O(g) + 1.5N2(g) + O2(g) → C3H5N3 O₂(1), AH = 1419.5 kJ Once reversed and normalized, rearrange the equation defining the enthalpy change for the reaction to solve for the heat of formation of nitroglycerin and substitute in known values: AH = ΣAH [products] - AH; [reactants] First launch this video. During the video, you'll be asked a conceptual question about the example. After watching the video, try the question again. You can watch the video again at any point.