For the reaction below:
a. Determine whether the reaction is energetically favorable at room temperature. Assume that ΔS=O. Calculate the gas phase enthalpy change using bond dissociation enthalpies at 25°C from the table below. Hint: Be aware that the bond energy for the C-H bond varies considerably and may change during the reaction; therefore, you will find several entries for C-H bonds in the table. Include the algebraic sign and specify units, e.g. -45 kJ/mol. Calculate to the nearest single energy unit.
b. Is the reaction exothermic
or endothermic?
Homework Answers
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For the reaction below: a. Determine whether the reaction is energetically favorable at room temperature. Assume that ΔS...
only problems f and h Energetics of Chemical Reactions 6.14 Using the table of average bond...
only problems f and h
Energetics of Chemical Reactions 6.14 Using the table of average bond dissociation enthalpies at 25°C, determine which of following reactions are energetically favorable at room temperature. Assume that AS Bond Dissociation Enthalpy kJ (kcal)/mol Bond Dissociation Enthalpy kJ (kcal)/mol Bond Bond Bond H-H 0-H C-H(-CH) C-HECH) C-HECH) N-H Si-H C-C 435 (104) 439 (105) 422 (101) 464 (111) 556 (133) 391 (93) 318 (76) 376 (90) 355 (85) 385 (92) C- C-Si CEC C= (aldehyde)...
Predict the enthalpy (ΔH) value for the theoretical reaction below, and indicate whether it is endothermic...
Predict the enthalpy (ΔH) value for the theoretical reaction below, and indicate whether it is endothermic or exothermic. The bond dissociation energy for each bond in Kcal/mol is shown below each reactant and product. (3p) A-B + C-D → A-C + B-D 63 88 47 96 A) +8 Kcal/mol, endothermic B) -8 Kcal/mol, exothermic C) +16 Kcal/mol, endothermic D) +8 Kcal/mol, exothermic
For the reaction below: CH4 •он CH3 H-OH a. Estimate the gas phase enthalpy change using...
For the reaction below: CH4 •он CH3 H-OH a. Estimate the gas phase enthalpy change using bond dissociation enthalpies from the OWL Table Reference, not data from your text. Click the References button and then click the Tables link on the drop-down that appears. Include algebraic sign and units. b. Is the reaction exothermic or endothermic? c. Is the reaction likely to proceed spontaneously in the direction written? For the reaction below: CH4 + Fz CH3-F H/F a. Estimate the...
2). Consider the following intramolecular S2 reaction. no ♡ + HI A) (5 pts) Use the...
2). Consider the following intramolecular S2 reaction. no ♡ + HI A) (5 pts) Use the table of Bond Dissociation Enthalpies (at the back of the exam) to calculate the approximate ΔΗπη. B) (3 pts) Is the reaction endothermic or exothermic? Why? C) (6 pts) Draw the Reaction Energy Coordinate Diagram. Label the axes, reactant(s), product(s), transition state(s), intermediate(s), activation energy, and reaction enthalpy. D) (3 pts) In regards to entropy, would you expect the reaction to be favorable, or...
For the reaction below CHy CH a. Estimate the gas phase enthalpy change using bond dissociation e...
For the reaction below CHy CH a. Estimate the gas phase enthalpy change using bond dissociation enthalpies from the OWL. Table Reference, not data from your text. button and then click the Tables link on the drop-down that appears. Include algebrakc sign and units b. Is the reaction exothermic or endothermic? c. Is the reaction likely to proceed spontaneously in the direction written? Submit Answer Retry Entire Group 1 more group attempt remaining 1 For the reaction below: a. Estimate...
BO D Which of ten The reaction of A to B. B) The reaction of B...
BO D Which of ten The reaction of A to B. B) The reaction of B to C. C) The reaction of C to D. D) All three steps occur at the same rate: there is no rate-limiting step. E) The most exothermic step is rate-limiting. esaretim Rank the following carbocations in order of stability. (The most stable is first.) > III II B) II > > III C) III > > II I > Il > III D 36)...
Draw curved arrows to show electron reorganization for the reaction step below. Arrow-pushing Instructions Visited GN=C:...
Draw curved arrows to show electron reorganization for the reaction step below. Arrow-pushing Instructions Visited GN=C: + Học : – GN=C–CH+ :: reg (References] Draw curved arrows to show electron reorganization for the reaction step below. Arrow-pushing Instructions Visited 210g 2re :o: H3c-c-c: :0-H :o: H3C-©-OH + :C: For the reaction below: H2C=CHCH2-H – OH H2C=CHCH2 + H-OH a. Estimate the gas phase enthalpy change using bond dissociation enthalpies from the OWL Table Reference, not data from your text. Click...
H-C=NO: HŇ=c=0 (a) Using bond enthalpies calculate the enthalpy of reaction. Assume the bond enthalpy of...
H-C=NO: HŇ=c=0 (a) Using bond enthalpies calculate the enthalpy of reaction. Assume the bond enthalpy of C=O listed in the table is true for this case. (b) Is this reaction endothermic or exothermic?
Use the References to access important values if needed for this question. For the reaction below:...
Use the References to access important values if needed for this question. For the reaction below: CHA + Fz CH;-F + H-F a. Estimate the gas phase enthalpy change using bond dissociation enthalpies from the OWL Table Reference, not data from your text. Click the References button and then click the Tables link on the drop-down that appears. Include algebraic sign and units. b. Is the reaction exothermic or endothermic? c. Is the reaction likely to proceed spontaneously in the...
Using the table of bond dissociation enthalpies, calculate AH° for the reaction A. (Use the entries...
Using the table of bond dissociation enthalpies, calculate AH° for the reaction A. (Use the entries for propene and propenyl halides for the calculation of cyclohexene and cyclohexenyl halides, respectively. Pay attention to the algebraic sign of your answer!) C-H bond BDE (kJ/mol) CH3-H 439 C2H:-H 422 (CH3), CH-H 414 (CH3)3C-H 405 CH2=CHCH2-H 372 CH2=CH-H 464 Table of bond dissociation enthalpies C-X bond BDE (kJ/mol) X, and HX bonds BDE (kJ/mol) CH3-I 242 CI-CI 247 C2H5-I 238 Br-Br 192 (CH3)2...
only problems f and h
Energetics of Chemical Reactions 6.14 Using the table of average bond dissociation enthalpies at 25°C, determine which of following reactions are energetically favorable at room temperature. Assume that AS Bond Dissociation Enthalpy kJ (kcal)/mol Bond Dissociation Enthalpy kJ (kcal)/mol Bond Bond Bond H-H 0-H C-H(-CH) C-HECH) C-HECH) N-H Si-H C-C 435 (104) 439 (105) 422 (101) 464 (111) 556 (133) 391 (93) 318 (76) 376 (90) 355 (85) 385 (92) C- C-Si CEC C= (aldehyde)...
For the reaction below: CH4 •он CH3 H-OH a. Estimate the gas phase enthalpy change using bond dissociation enthalpies from the OWL Table Reference, not data from your text. Click the References button and then click the Tables link on the drop-down that appears. Include algebraic sign and units. b. Is the reaction exothermic or endothermic? c. Is the reaction likely to proceed spontaneously in the direction written? For the reaction below: CH4 + Fz CH3-F H/F a. Estimate the...
2). Consider the following intramolecular S2 reaction. no ♡ + HI A) (5 pts) Use the table of Bond Dissociation Enthalpies (at the back of the exam) to calculate the approximate ΔΗπη. B) (3 pts) Is the reaction endothermic or exothermic? Why? C) (6 pts) Draw the Reaction Energy Coordinate Diagram. Label the axes, reactant(s), product(s), transition state(s), intermediate(s), activation energy, and reaction enthalpy. D) (3 pts) In regards to entropy, would you expect the reaction to be favorable, or...
For the reaction below CHy CH a. Estimate the gas phase enthalpy change using bond dissociation enthalpies from the OWL. Table Reference, not data from your text. button and then click the Tables link on the drop-down that appears. Include algebrakc sign and units b. Is the reaction exothermic or endothermic? c. Is the reaction likely to proceed spontaneously in the direction written? Submit Answer Retry Entire Group 1 more group attempt remaining 1 For the reaction below: a. Estimate...
BO D Which of ten The reaction of A to B. B) The reaction of B to C. C) The reaction of C to D. D) All three steps occur at the same rate: there is no rate-limiting step. E) The most exothermic step is rate-limiting. esaretim Rank the following carbocations in order of stability. (The most stable is first.) > III II B) II > > III C) III > > II I > Il > III D 36)...
Draw curved arrows to show electron reorganization for the reaction step below. Arrow-pushing Instructions Visited GN=C: + Học : – GN=C–CH+ :: reg (References] Draw curved arrows to show electron reorganization for the reaction step below. Arrow-pushing Instructions Visited 210g 2re :o: H3c-c-c: :0-H :o: H3C-©-OH + :C: For the reaction below: H2C=CHCH2-H – OH H2C=CHCH2 + H-OH a. Estimate the gas phase enthalpy change using bond dissociation enthalpies from the OWL Table Reference, not data from your text. Click...
H-C=NO: HŇ=c=0 (a) Using bond enthalpies calculate the enthalpy of reaction. Assume the bond enthalpy of C=O listed in the table is true for this case. (b) Is this reaction endothermic or exothermic?
Use the References to access important values if needed for this question. For the reaction below: CHA + Fz CH;-F + H-F a. Estimate the gas phase enthalpy change using bond dissociation enthalpies from the OWL Table Reference, not data from your text. Click the References button and then click the Tables link on the drop-down that appears. Include algebraic sign and units. b. Is the reaction exothermic or endothermic? c. Is the reaction likely to proceed spontaneously in the...
Using the table of bond dissociation enthalpies, calculate AH° for the reaction A. (Use the entries for propene and propenyl halides for the calculation of cyclohexene and cyclohexenyl halides, respectively. Pay attention to the algebraic sign of your answer!) C-H bond BDE (kJ/mol) CH3-H 439 C2H:-H 422 (CH3), CH-H 414 (CH3)3C-H 405 CH2=CHCH2-H 372 CH2=CH-H 464 Table of bond dissociation enthalpies C-X bond BDE (kJ/mol) X, and HX bonds BDE (kJ/mol) CH3-I 242 CI-CI 247 C2H5-I 238 Br-Br 192 (CH3)2...
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