37) Use bond energies to calculate the enthalpy changes for the formation of ethane(C;H6) from ethylene (C3Ha) and hydrogen (H2). Bond energies: H'(kJ/mol):(C-H): 413, (C-C): 614, (C-C): 348, (H-H): 446. Is the reaction endo orexothermic ?H HH-c-C-HC=cH-HH Ha) - 114b) + 114c) - 230d) +330

The reaction taking place is given by, => H2C=CH2 + H-H ------> H3C-CH3

37) Use bond energies to calculate the enthalpy changes for the formation of ethane (C:H.) from ethylene (CHa) and hydrogen (H2). Bond energies: H'(kJ/mol): (C-H): 413, (C-C): 614, (C-C): 348, (H-H): 446. Is the reaction endo or exothermic ? H H H-c-C-H C=C H-H H H a) - 114 b) + 114 c) - 230 d) + 330

37) Use bond energies to calculate the enthalpy changes for the formation of ethane (C:H.) from ethylene (CHa) and hydrogen (H2). Bond energies: H'(kJ/mol): (C-H): 413, (C-C): 614, (C-C): 348, (H-H): 446. Is the reaction endo or exothermic ? H H H-c-C-H C=C H-H H H a) - 114 b) + 114 c) - 230 d) + 330

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter9: Chemical Bonds

Section: Chapter Questions

Problem 9.89QE

See similar textbooks

Similar questions

Write the chemical formula and Lewis structure of the following each of which contains five carbon atoms: (a) an alkane. (b) an alkene. (c) an alkyne
Use average bond energies to calculate ΔHrxnΔHrxn for the following hydrogenation reaction: H2C=CH2(g)+H2(g)→H3C−CH3(g)
Q1 The balanced equation for the fomplete combustion of acetone(C3H6O) is: C3H6O + 4O2 --> 3CO2 + 3H2O ΔrH-1790kJmol^-1 If a bottle of nail polish remover contains 177mL of avetone(density 0.788gmL^-1) how much heat is released by its complete combustion? Q2. Draw the lewis structures for O-N-Cl and N-O-Cl. calculate the formal charges of the atoms and use these to determine which of these isomers is more stable. Q3. The work function of aluminum is 412kJmol^-1. If light corresponding to 471kJ mol^-1 is shone on the metal what is the velocity of the electrons that are emitted from the metal?
Acetylene (C2H2) and nitrogen (N2) both contain a triplebond, but they differ greatly in their chemical properties.(a) Write the Lewis structures for the two substances. (b) By referring to Appendix C, look up the enthalpies of formationof acetylene and nitrogen. Which compound is more stable?(c) Write balanced chemical equations for the completeoxidation of N2 to form N2O5(g) and of acetylene to formCO2(g) and H2O(g). (d) Calculate the enthalpy of oxidationper mole for N2 and for C2H2 (the enthalpy of formationof N2O5(g) is 11.30 kJ/mol). (e) Both N2 and C2H2 possesstriple bonds with quite high bond enthalpies (Table 8.3).Calculate the enthalpy of hydrogenation per mole for bothcompounds: acetylene plus H2 to make methane, CH4;nitrogen plus H2 to make ammonia, NH3.
Octane (C8H18) is combusted with oxygen to give carbon dioxide and water vapor. Calculate the enthalpy of reaction using the bond energies given. Is the combustion of octane an endothermic or exothermic reaction? The reaction below is not balanced. pleaseanswer neatly so i can see how to do it Bond: C=O O=O C–H O–H C–C Bond energy (kJ/mol): 799 498 414 464 347
How many grams of CO2 are produced when C3H8 is combusted in oxygen and 507.0 kJ of heat are released? Estimate ΔHrxn using bond enthalpies from the table above in order to solve this problem. Bond Bond Energy (kJ/mol) Bond Bond Energy (kJ/mol) C-C 347 C=O (in CO2) 799 C=C 614 C=O 745 C≡C 839 C≡O 1070 C-H 413 O=O 498 O-H 467 N-H 391 H-H 432 N≡N 945 C-O 358 N-Cl 200 C-N 305 N-O 201 C-Cl 339 C≡N 891
what are other reasonable structures and which one is the most stable?
Estimate the carbon–fluorine bond energy given that the C-C bond energy is 347 kJ/mol, the C=C bond energy is 614 kJ/mol, and the F-F bond energy is 154 kJ/mol. Delta H = -549 kJ
Using the table of bond energies above, estimate the enthalpy change (kJ) for the following reaction: 2NCl3(g)⟶N2(g)+3Cl2(g) Bond Bond Energy (kJ/mol) Bond Bond Energy (kJ/mol) C-C 347 C=O (in CO2) 799 C=C 614 C=O 745 C≡C 839 C≡O 1070 C-H 413 O=O 498 O-H 467 N-H 391 H-H 432 N≡N 945 C-O 358 N-Cl 200 C-N 305 N-O 201 C-Cl 339 C≡N 891 Cl-Cl 243 S-Cl 250 S=O 535 S-S 215 S-O 364 S-H 339
Using the table of bond energies below, estimate the enthalpy change (kJ) for the following reaction: CH4+2O2⟶CO2+2H2O Bond Bond Energy (kJ/mol) Bond Bond Energy (kJ/mol) C-C 347 C=O (in CO2) 799 C=C 614 C=O 745 C≡C 839 C≡O 1070 C-H 413 O=O 498 O-H 467 N-H 391 H-H 432 N≡N 945 C-O 358 N-Cl 200 C-N 305 N-O 201 C-Cl 339 C≡N 891 Cl-Cl 243
If the first, second and third bond dissociation enthalpies of methane are +420, +475, and +421 KJmol-l, respectively, calculate the fourth. How do you account for the fact that; ammonium nitrate is readily soluble in water even though the standard enthalpy of solution has a positive value? although the enthalpy of combustion of cane sugar is about -6000 KJmol-l cane sugar is not observed to oxidise in air at ordinary temperature?
Define bond energy using the H--Cl bond as an example.When this bond breaks, is energy absorbed or released? Is the accompanying ΔH value positive or negative? How do the mag-nitude and sign of this ΔH value relate to the value that accom-panies H--Cl bond formation?