The average bond enthalpy for c-h is 413 kj/mol. 413 kj of energy is required to break a mole of ch into atoms: ch (g) →c (g) + h (g), δh=413 kj using this information, and your answer from part a, calculate the enthalpy change of the reaction from part

b. that is, calculate the energy required to break only the carbon-carbon bonds in benzene. express your answer to four significant figures and include the appropriate units.

Question

Nikolai Montgomery

Chemistry

8 October, 06:57

The average bond enthalpy for c-h is 413 kj/mol. 413 kj of energy is required to break a mole of ch into atoms: ch (g) →c (g) + h (g), δh=413 kj using this information, and your answer from part a, calculate the enthalpy change of the reaction from part

b. that is, calculate the energy required to break only the carbon-carbon bonds in benzene. express your answer to four significant figures and include the appropriate units.

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Jaylah Jennings · Answer 1

To compute for the energy essential to break only the carbon-carbon bonds in benzene. The solution would be:ΔH = 413 kJ, there are 6CH which is the answer is part b. 413 * 6 = 2478 kJ ΔHrxn = 5535 kJ is the answer in part a. The answer would be: 5535-2478 = 3057 kJ [or 3060 kJ rounded off into 4 sig figs]