▼ Part A The C-H bond in CH4. Express your answers in kilojoules per mole to three significant figures separated by a comma. 195] ΑΣΦ Bond enthalpy, bond energy = Submit Request Answer Part B Bond enthalpy, bond energy- The C-C single bond in C3H6 (cyclopropane) (use C-H bond enthalpy and bond energy calculated for CH₂). Express your answers in kilojoules per mole to three significant figures separated by a comma. 195] ΑΣΦ Submit Request Answer Part C ? Bond enthalpy, bond energy- ? kJ-mol-1 ? The CC double bond in C₂H₁ (use C-H bond enthalpy and bond energy calculated for CH₂). Express your answers in kilojoules per mole to three significant figures separated by a comma. 195] ΑΣΦΑ kJ-mol-1 kJ mol

▼ Part A The C-H bond in CH4. Express your answers in kilojoules per mole to three significant figures separated by a comma. 195] ΑΣΦ Bond enthalpy, bond energy = Submit Request Answer Part B Bond enthalpy, bond energy- The C-C single bond in C3H6 (cyclopropane) (use C-H bond enthalpy and bond energy calculated for CH₂). Express your answers in kilojoules per mole to three significant figures separated by a comma. 195] ΑΣΦ Submit Request Answer Part C ? Bond enthalpy, bond energy- ? kJ-mol-1 ? The CC double bond in C₂H₁ (use C-H bond enthalpy and bond energy calculated for CH₂). Express your answers in kilojoules per mole to three significant figures separated by a comma. 195] ΑΣΦΑ kJ-mol-1 kJ mol

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter2: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 2.93E: Find the enthalpies of the combustion reactions for methane through n-octane. Plot them versus the...

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From the following enthalpies of reaction, 4HCl(g) + O2(g) -> 2H2O(l) + 2Cl2(g) ΔH = -202.4 kJ/mol rxn 1/2 H2(g) + 1/2 F2(g) -> HF(l) ΔH = -600.0 kJ/mol rxn H2(g) + 1/2 O2(g) -> H2O(l) ΔH = -285.8 kJ/mol rxn find ΔHrxn (in kJ/mol) for 2HCl(g) + F2(g) -> 2HF(l) + Cl2(g). Final answer: (4 significant figures)
Given the following information: C(s) + 02(g) ---> C02(g) delta H= -393.5 kJ H2(g) + 1/2 02(g)--> H20(I) delta H= -285.8 kJ C2H2(g) + 5/2 02(g)--> 2 C02(g) + H20(I) delta H= -1299.8 kJ find the enthalpy change for: 2 C(s) + H2(g)--> C2H2(g) a.) -454.0 kJ b.) -227.0 kJ c.) 0.0 kJ d.) 227.0 kJ e.) 454.0 kJ
Calculate the enthalpy of combustion (in kj) of methyl linoleate (c19h34o2) an important component of many biodiesel fuels made from corn oil and methanol, given the following standard ethalpies of formation: CO2(g)=-393.5kj/mol H2O(l)=-285.8kj/mol C19H34O2(l)=-645.7kj/mol
Some bacteria can obtain energy for growth by oxidizing ethanol, first to acetaldehyde and then acetic acid. Calculate ΔH° for the reaction:(a) C2H5OH(l) + ½O2(g) ---> CH3CHO(l) + H2O(l)Use the following enthalpies of combustion: ΔcH°(C2H5OH, l) = -1362.8 kJ mol-1, ΔcH°(CH3CHO, l) = -886.8 kJ mol-1
(a) The heats of atomization of ethane and propane are +2824KJ/mol and +3996KJ/mol respectively. Calculate the bond energies of C-C and C-H. (b) Given the following bond energies H-H = +435KJ/mol , C=C = +619KJ/mol, and your values obtained for C-C and C-H in (a) above, calculate the standard molar enthalpy change for the reaction CH2=CH2 + H2 C2H6
Calculate the enthalpy for the reaction, BaC₂ (s) + 2 H₂O (l) → Ba(OH)₂ (aq) + C₂H₂ (g) Using the appropriate data from the following reactions, Ba (s) + 2 C (graphite, s) → BaC₂ (g) ∆H° = +437 kJ/mol Ba (s) + 2 H₂O (l) → Ba(OH)₂ +H₂ (g) ∆H° = -374.7 kJ/mol Ba (s) + 1/2 O₂ (g) → BaO (s) ∆H° = -553.5 kJ/mol BaO (s) + H₂O (l) → Ba(OH)₂ (aq) ∆H° = -107 kJ/mol C₂H₂ (g) + 5/2 O₂ (g) → 2 CO₂ (g) + H₂O (l) ∆H° = -1300. kJ/mol C (graphite, s) + O₂ (g) → CO₂ (g) ∆H° = -393.5 kJ/mol H₂ (g) + 1/2 O₂ (g) → H₂O (l) ∆H° = -285.8 kJ/mol
Given the following standard enthalpies; H2(g) ➡ 2H(g) △H = +436KJ O2(g) ➡ 2O(g) △H = +498KJ Hf = -285 KJ/mol Calculate the O-H bond enthalpy in water, as fast as possible explaining clearly your steps.
3. Using standard enthalpies of formation (∆Hfº), calculate the enthalpy change for the following reaction: 2H2S(g) + 3O2(g) → 2H2O(l) + 2SO2(g) ∆Hrxn = ? ΔHf H2S (g) = -39.0 kJ/mol ΔHf O2 (g) = 0.0 kJ/mol ΔHf H2O (l) = -285.8 kJ/mol ΔHf SO2 (g) = -296.8 kJ/mol
Calculate the enthalpy of combustion for kerosene. Assume that kerosene is C10H22(l) and that the products are CO2(g) and H2O(l). ΔH°f (C10H22(l)) = –249.6 kJ/mol ΔH°f (CO2(g)) = –393.5 kJ/mol ΔH°f (H2O(l)) = –285.8 kJ/mol Select one: a. –872.9 kJ/mol b. –5489.9 kJ/mol c. –429.7 kJ/mol d. –6829.2 kJ/mol
Draw a (hess diagram) enthalpy diagram to calculate the ∆Hfc2 H5 OH using the following date ∆Hcc = -393.5 KJ mol-1 ∆HcH2 = -285.8 KJ mol-1 ∆Hc2H5OH = -1367.3KJ mol-1
Given the following data: C2H4(g) + 3 O2(g) → 2 CO2(g) + 2 H2O(l) DH = -1411.0 kJ 2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(l) DH = -3120.0 kJ 2 H2(g) + O2(g) → 2 H2O(l) DH = -571.6 kJ Calculate the enthalpy of the reaction: C2H4(g) + H2(g) → C2H6(g) DH = ___ kJ
The combustion of ammonia is : 4NH3(g)+5O2(g)--> 4NO(g)+6H2O(g) DeltaH= -905kJ what is the enthalpy of the formation (kJ/mol) of NH3(g) [Heat of formation data: NO(g)=90.4 kJ/ mol, H2O(g)=-241 kJ/mol]