Answered: The Explosive Nitroglycerin (C3H5N3O9)… | Bartleby

Skip to main contentcloseHomework Help is Here – Start Your Trial Now!arrow_forwardSEARCHHomework help starts here!ASK AN EXPERTASKScienceChemistryThe explosive nitroglycerin (C3H5N3O9) decomposes rapidly upon ignition or sudden impact according to the following unbalanced equation: C3H5N3O9(l)  CO2(g) + H2O(g) + N2(g) + O2(g) ∆H o = -5678 kJ Calculate the standard enthalpy of formation of nitroglycerin.The explosive nitroglycerin (C3H5N3O9) decomposes rapidly upon ignition or sudden impact according to the following unbalanced equation: C3H5N3O9(l)  CO2(g) + H2O(g) + N2(g) + O2(g) ∆H o = -5678 kJ Calculate the standard enthalpy of formation of nitroglycerin.BUYChemistry 10th EditionISBN: 9781305957404Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher: Cengage Learningexpand_less1 Chemical Foundations2 Atoms, Molecules, And Ions3 Stoichiometry4 Types Of Chemical Reactions And Solution Stoichiometry5 Gases6 Thermochemistry7 Atomic Structure And Periodicity8 Bonding: General Concepts9 Covalent Bonding: Orbitals10 Liquids And Solids11 Properties Of Solutions12 Chemical Kinetics13 Chemical Equilibrium14 Acids And Bases15 Acid-base Equilibria16 Solubility And Complex Ion Equilibria17 Spontaneity, Entropy, And Free Energy18 Electrochemistry19 The Nucleus: A Chemist's View20 The Representative Elements21 Transition Metals And Coordination Chemistry22 Organic And Biological Moleculesexpand_moreChapter Questionsexpand_moreProblem 1RQProblem 2RQProblem 3RQProblem 4RQProblem 5RQProblem 6RQProblem 7RQProblem 8RQProblem 9RQProblem 10RQProblem 1ALQProblem 2ALQProblem 3ALQProblem 4ALQProblem 5ALQProblem 6ALQProblem 7ALQProblem 8ALQProblem 9ALQProblem 10ALQProblem 11ALQProblem 14ALQProblem 15ALQProblem 16ALQProblem 17ALQProblem 18ALQProblem 19QProblem 20QProblem 21QProblem 22QProblem 23QProblem 24QProblem 25QProblem 26QProblem 28QProblem 29QProblem 30QProblem 31EProblem 32EProblem 33EProblem 34EProblem 35EProblem 36EProblem 37EProblem 38EProblem 39EProblem 40EProblem 41EProblem 42EProblem 43EProblem 44EProblem 45EProblem 46EProblem 47EProblem 48EProblem 49EProblem 50EProblem 51EProblem 52EProblem 53EProblem 54EProblem 55EProblem 56EProblem 57EProblem 58EProblem 59EProblem 60EProblem 61EProblem 62EProblem 63EProblem 64EProblem 65EProblem 66EProblem 67EProblem 68EProblem 69EProblem 70EProblem 71EProblem 72EProblem 73EProblem 74EProblem 75EProblem 76EProblem 77EProblem 78EProblem 79EProblem 80EProblem 81EProblem 82EProblem 83EProblem 84EProblem 85EProblem 86EProblem 87EProblem 88EProblem 89EProblem 90EProblem 91EProblem 92EProblem 93AEProblem 94AEProblem 95AEProblem 96AEProblem 97AEProblem 98AEProblem 99AEProblem 100AEProblem 101AEProblem 102AEProblem 103AEProblem 104AEProblem 105AEProblem 106AEProblem 107AEProblem 108AEProblem 109AEProblem 110AEProblem 111CWPProblem 112CWPProblem 113CWPProblem 114CWPProblem 115CWPProblem 116CWPProblem 117CPProblem 118CPProblem 119CPProblem 120CPProblem 121CPProblem 122CPProblem 123CPProblem 124CPProblem 125CPformat_list_bulletedSee similar textbooks

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12. The explosive nitroglycerin (C3H5N3O9) decomposes rapidly upon ignition or sudden impact according to the following unbalanced equation: C3H5N3O9(l)  CO2(g) + H2O(g) + N2(g) + O2(g) ∆H o = -5678 kJ Calculate the standard enthalpy of formation of nitroglycerin.

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See solutionCheck out a sample Q&A hereKnowledge BoosterLearn more about ThermodynamicsNeed a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questionsarrow_back_iosarrow_forward_ios

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• A scientist measures the standard enthalpy change for the following reaction to be 209.4 kJ : CHĄ(g) + H20(g)3H2(g) + CO(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of CH4(g) is kJ/mol.arrow_forwardThe enthalpy of decomposition of NO₂Cl is -114.0 kJ. Use the following data to calculate the heat of formation of NO₂Cl from N₂, O₂, and Cl₂: ✓ NO₂Cl(g) →→→ NO₂(g) + Cl₂ (g) ½-½N₂(g) + O₂(g) → NO₂(g) N₂(g) + O₂(g) + Cl₂(g) →→ NO₂CI (g) 1st attempt kJ AH rxn=-114.0 kJ AH = +33.2 kJ AH = ? See Periodic Table See Hintarrow_forwardWhen HCI(g) reacts with O₂(g) according to the following reaction, 28.6 kJ of energy are evolved for each mole of HCI(g) that reacts. Complete the following thermochemical equation. 4HCI(g) + O₂(g)2H₂O(g) + 2Cl₂(g) ΔΗ = 28.6| kjarrow_forward
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