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Science

Chemistry

J Δ

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 2E: Prepare a table identifying several energy transitions that take place during the typical operation...

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Diels Alder Cycloaddition: Focus on regiochemistry (problems E-F) –> match + of the
dienophile and - of the diene while also considering stereochemistry (endo).

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Given the following data: C2H4(g) + 3O2(g) -> 2CO2(g) +2H2O(l) deltaH = -1411.0 kJ 2C2H6(g) + 7O2(g) -> 4CO2(g) +6H2O(l) deltaH = -3119.8 kJ 2H2(g) +O2 -> 2H2O(l) deltaH = -571.7 kJ Calculate deltaH for the reaction: C2H4(g) + H2(g) -> C2H6(g)
2. Given the following data: P4(s) + 6CI2(g) →> 4PCI3(g) AHrxn = 1225.6 kJ %3D P4(s) + 502(g) →> P4O10(s) AHrxn = -2967.3 kJ %3D PCI3(g) + Cl2(g)→ PCI5(g) AHrxn = -84.2 kJ %3D PCI3(g) + %02(g) → CI3PO(g) AHrxn = -285.7 kJ %3D Calculate AH for the reaction P4O10(s) + 6PCI5(g) → 10C13PO(g)
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
Use average bond energies to compare the stabilities of allyl alcohol, CH2CHCH2OH, and acetone, (CH3)2CO, both of which have the same formula, C3H60. What is the difference in stabilities of the two compounds? Give the absolute value of the difference (positive value). i kJ eTextbook and Media Select all that apply to the stability of allyl alcohol and acetone. O Allyl alcohol is more stable due to difference in stabilities. O Acetone is more stable due to difference in stabilities. O Acetone is more stable than allyl alcohol. O Allyl alcohol is more stable than acetone.
Given the following data: C2H2(g) + 5/2 O2(g) --> 2CO2(g) + H2O(l) ΔH= -1300.kJ C(s) + O2(g) --> CO2(g) ΔH= -394kJ H2(g) + 1/2O2(g) --> H2O(l) ΔH= -286kJ Use Hess’s Law to calculate ΔH for the reaction 2C(s) + H2(g) --> C2H2(g)
Calculate AH for the reaction: C2H4 (g) + H2 (g) → C2H6 (g), from the following data: C2H4 (g) + 3 O2 (g) → 2 CO2 (g) + 2 H2O (I) AH = -1411. kJ/mol 2 C2H6 (g) + 7 O2 (g) → 4 CO2 (g) + 6 H2O (1) AH = -3120. kJ/mol 2 H2 (g) + O2 (g) → 2 H20 (1) AH = -571.6 kJ/mol Select one: O - 136.8 kJ/mol O 1137 kJ/mol O -273.6 kJ/mol O 133.3 kJ/mol
C2H5OH(l)+3O2(g)→2CO2(g)+3 H2O(l)ΔH∘2=−1370kJ/molrxnC2H5OH(l)+3⁢O2(g)→2CO2(g)+3 H2O(l)ΔH2∘=−1370kJ/molrxn (c) Based on the information above, identify the ΔH∘ΔH∘ values that should be added together to determine the value of ΔH∘rxnΔHrxn∘ for the following reaction. C2H4(g)+H2O(l)→C2H5OH(l)
Provided the following information determine AH formation of C2H6(g). C(graphite) + O2(g) CO2(g) AH = -393.5 kJ > H2(g) + O2(g) – H2O(I) AH = -285.8 kJ C2Ho(g) + 02(g) – 2CO2(g) + 3H2O() ΔΗ = -1560.7 kJ
A cubic piece of uranium metal (specific heat capacity = 0.117 J/C g) at 200.0C is dropped into 1.00 L deuterium oxide ("heavy water;" specific heat capacity = 4.21 I J/C g) at 25.5C. The final temperature of the uranium and deuterium oxide mixture is 28.5C. Given the densities of uranium (19.05 g/cm3) and deuterium oxide (1.11 g/mL). what is the edge length of the cube of uranium?
Provided the following information determine delta Hformation of C2H6(g). C(graphite) + O2(g) -> CO2(g) delta H = -393.5 kJ H2(g) + 1/2 O2(g) -> H2O(l) delta H = -285.8kj C2H6(g) + 7/2 O2(g) -> 2CO2(g) + 3H2O(l) delta H = -1560.7 kj
Given the following data: Fe203(s) + 3CO(g) → 2Fe(s) + 3CO2(g) AH = - :-23 kJ 3Fe,O3(s) + CO(g) → 2Fe;O4(s) + CO2(g) AH=-39 kJ Fe;04(s) + CO(g) → 3FEO(s) + CO2(g) AH = 18 kJ calculate AH value for the reaction FeO(s) + CO(g) → Fe(s) + CO2(g) ΔΗ- kJ
Where c-h: 413, c=c: 614, o-h:467, c-c: 347, c-o:358