Question

Calculate the average C—C bond strength in cyclopropane (in kJ/mol). Its combustion and the experimental enthalpy...

Calculate the average C—C bond strength in cyclopropane (in kJ/mol). Its combustion and the experimental enthalpy of reaction are:

C3H6(g) + 4.5O2(g) → 3CO2(g) + 3H2O(g) ΔHºrxn = -1,957.7 kJ/mol

Average bond strentgh (kj/mol):

O - H = 463

C - H = 414

C - C = 347

O -- O = 498 (DOUBLE BOND)

C -- O = 745 (DOUBLE BOND)

C -- O (CO2 = 799)

Since all reactants and products are in the gaseous state, bond energies may be used to estimate the enthalpy of reaction. Do not use the standard C—C bond strength, leave the C—C bond strength as an unknown and solve for its value.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The enthalpy of combustion ΔcH° of gaseous cyclopropane, C3H6, is -2091 kJ mol-1 at 25 °C....
The enthalpy of combustion ΔcH° of gaseous cyclopropane, C3H6, is -2091 kJ mol-1 at 25 °C. a. What is the standard enthalpy of formation of cyclopropane? b. What is the standard internal energy change of combustion of cyclopropane at 25 °C. c. Using heat capacity values in the back of your book, what is the standard enthalpy of combustion of cyclopropane at 100 °C? d. Again using heat capacity values in the back of your book, what is the standard...
Ethane undergoes a combustion reaction. Using the following bond strengths, please calculate the enthalpy of reaction....
Ethane undergoes a combustion reaction. Using the following bond strengths, please calculate the enthalpy of reaction. C – H bond = 413 kJ/mole C = O bond = 799 kJ/mole H – O bond = 463 kJ/mole O = O bond = 495 kJ/mole C – O bond = 358 kJ/mole O – O bond = 146 kJ/mole C – C bond = 346 kJ/mole A. About -2800 kJ B. About 2800 kJ C. About -1500 kJ D. About 1500...
Using the bond enthalpies in the Average Bond Enthalpies table, determine the approximate enthalpy (in kJ)...
Using the bond enthalpies in the Average Bond Enthalpies table, determine the approximate enthalpy (in kJ) for each of the following reactions. (Assume the average bond enthalpy of the Cl–F bond is 254 kJ/mol.) C) 2 CH3(C=O)H(g) + 5 O2(g) → 4 CO2(g) + 4 H2O(g)
Data Tables Heats of Formation Compound delta Hf (kJ mol-1) H20 (l) -285.83 CO2 (g) -391.51...
Data Tables Heats of Formation Compound delta Hf (kJ mol-1) H20 (l) -285.83 CO2 (g) -391.51 Bond Enthalpies Reaction delta H (298K) C(s, graphite) to C(g) 716.7 H-H to 2H(g) 436 C-H to C(g) + H(g) 413 C-C to 2C(g) 348 *****For the word "to" it means arrow, or reacts to form this (not able to put an arrow on here) a) If the standard enthalpy of combustion of gaseous cyclopropane, C3H6, is -2091.2kJ mol-1 at 25 C, calculate the...
Estimate the carbon-carbon bond strength in benzene given: 2C6H6(g)+15O2(g)⟶12CO2(g)+6H2O(g)  ΔH∘=−6339kJ Bond dissociation data are the following: the...
Estimate the carbon-carbon bond strength in benzene given: 2C6H6(g)+15O2(g)⟶12CO2(g)+6H2O(g)  ΔH∘=−6339kJ Bond dissociation data are the following: the strength of the O=O bond in O2 is 498 kJ/mol, the strength of the C=O bond in CO2 is 804 kJ/mol, the strength of the H−O bond in H2O is 460 kJ/mol, the strength of the H−C bond in benzene is 410 kJ/mol.
1. Use the average bond enthalpies from the table to calculate the overall ΔH for this...
1. Use the average bond enthalpies from the table to calculate the overall ΔH for this reaction. Hint: Don't forget the C-C bond in CH3CH3. 2 CH3CH3 + 7 O2 → 4 CO2 + 6 H2O Selected Average Bond Energies Bond Avg. Bond Energy (kJ/mol) Bond Avg. Bond Energy (kJ/mol) C-H 415 H-H 436 C-C 350 H-O 464 C=C 611 H-N 389 C-O 360 N-O 222 C=O 736 N2 946 C=O in CO2 804 Cl2 243 C-N 305 Br2 193...
Calculate in kJ/mol the enthalpy of combustion for citric acid using bond energies. Draw out structures...
Calculate in kJ/mol the enthalpy of combustion for citric acid using bond energies. Draw out structures to indicate where bonds are breaking/forming.
The combustion of methane, CH4, releases 890.4 kj/mol of heat. That is, when one mole of...
The combustion of methane, CH4, releases 890.4 kj/mol of heat. That is, when one mole of methane is burned, 890.4 kj are give off to the surroundings. This means that the products have less energy stored in the bonds than the reactants. Thus, for the reaction: CH4(G) + 2 O (g) -> CO2 (g) + 2 H2O (I) deltaH= -890.4kj/mol. A) what is the enthalpy change when 2.00 mol of CH4 are burned? B)what is the enthalpy change when 22.4g...
What is the heat of combustion (Δ H ° rxn ) for acetylene (C 2 H...
What is the heat of combustion (Δ H ° rxn ) for acetylene (C 2 H 2 ) , assuming that the combustion products are CO 2 ( g ) and H 2 O( g ). Hint make sure to balance the equation. Instead of determining heats of reaction from heats of formation we sometime use average bond dissociation energies to calculate heats of reaction. Why would we need to use bond dissociation energies and how would your formula change?...
____ 1. To conduct an experiment, a scientist places a small piece of aluminum in a...
____ 1. To conduct an experiment, a scientist places a small piece of aluminum in a test tube and adds sodium hydroxide solution. Bubbles of gas are produced and the outside of the test tube becomes hot to the touch. Which of the following is true? The reaction is endothermic, and the system gains energy from the surroundings. The reaction is exothermic, and the system loses energy to the surroundings. The reaction is endothermic, and the system loses energy to...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT