Draw the HEXAGONAL skeletal (bond - line) structure of a hydrocarbon containing a substituted five-membered ring with one double bond ( cyclopentene) with the following molecular formula of C6H10. C-H bonds are implied show work

Draw the structures of 1,3-pentadiene and 1,4-pentadiene and label the carbons. Predict the trendin C-C single bond lengths in the two compounds.

Carbon–carbon bond dissociation enthalpies have been measured for many alkanes. Identify the alkane in each of the following pairs that has the lower carbon–carbon bond-dissociation enthalpy, and explain the reason for your choice. (a) Ethane or propane (b) Propane or 2-methylpropane (c) 2-Methylpropane or 2,2-dimethylpropane (d) Cyclobutane or cyclopentane

Using the provided bond energies, estimate the AHrxn for the generic reaction below. The skeletal structures of each molecule are shown below the balanced equation, where each (-) represents a single bond. 2 A2 B → 2 A2 + B2 2 (A – B – A) → 2 (A – A) + (B – B) - - Bond energies: (A-B) = 150. kJ/mol; (A-A) = 200. kJ/mol; (B-B) %3D = 250. kJ/mol O -300. kJ O 350. kJ O -50. kJ 600. kJ O 1250. kJ

Hi! I found some answers for this question but I am not sure about it.Can you explain the question?

(a) The heats of atomization of ethane and propane are +2824KJ/mol and +3996KJ/mol respectively. Calculate the bond energies of C-C and C-H. (b) Given the following bond energies H-H = +435KJ/mol , C=C = +619KJ/mol, and your values obtained for C-C and C-H in (a) above, calculate the standard molar enthalpy change for the reaction CH2=CH2 + H2          C2H6

(a) The heats of atomization of ethane and propane are +2824KJ/mol and +3996KJ/mol respectively. Calculate the bond energies of C-C and C-H. (b) Given the following bond energies H-H = +435KJ/mol , C=C = +619KJ/mol, and your values obtained for C-C and C-H in (a) above calculate the standard molar enthalpy change for the reaction CH2=CH2 + H2        to yield  C2H6

A.) What is the heat of reaction, ΔH°? CO2(g) + H2O(l) à H2CO3(aq)   –20.2 kJ mol–1   –1379 kJ mol–1   –592 kJ mol–1 B.)  What is the average bond energy in CO2? CO2(g)          ΔH°f, = –393.5 kJ mol–1 CO(g)           ΔH°f, = –110.5 kJ mol–1 C(g)              ΔH°f, = +715 kJ mol–1        CO32–(aq)      ΔH°f, = –676.3 kJ mol–1 O(g)               ΔH°f, = +249.0 kJ mol–1   207 kJ mol–1   1607 kJ mol–1   804 kJ mol–1

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Find the enthalpy of combustion of 1 mole of propane, CH3CH2CH3.  Here are some bond enthalpy values: C-H=413 C-O= 358 O-H=436 C=(double bond)O=804 C-C=348 O=O=498