Some lipids contains carbon to carbon double bonds.Given the bond dissociation energies in the table, calculate the enthalpy change when one mole of hydrogen is added across one double bond. A.+1520 kJ/molB.-1520 kJ/molC.+120 kJ/molD.-120 kJ/mol
Question
Some lipids contains carbon to carbon double bonds.Given the bond dissociation energies in the table, calculate the enthalpy change when one mole of hydrogen is added across one double bond. A.+1520 kJ/molB.-1520 kJ/molC.+120 kJ/molD.-120 kJ/mol
Solution
To answer this question, we need more information. Specifically, we need the bond dissociation energies for the relevant bonds. The question mentions a table, but the table is not provided.
In general, the enthalpy change (ΔH) for a reaction can be calculated using the formula:
ΔH = Σ(Bond energies of bonds broken) - Σ(Bond energies of bonds formed)
In this case, we are breaking a carbon-carbon double bond and forming two carbon-hydrogen bonds. So, we would need the bond dissociation energies for these bonds to calculate the enthalpy change.
Once we have those values, we can substitute them into the formula to find the answer.
Without the specific bond dissociation energies, we cannot determine whether the enthalpy change is +1520 kJ/mol, -1520 kJ/mol, +120 kJ/mol, or -120 kJ/mol.
Similar Questions
Given the following bond dissociation energies, calculated the enthalpy of the following reaction.H-C≡C-H + 2H2 → H3C-CH3C-C 350 kJ/molC≡C 807 kJ/molC-H 410 kJ/molH-H 436 kJ/molHint: There are 2 H-H bonds on the left and a total of 6 C-H bonds on the right.Group of answer choices-111 kJ/mol-211 kJ/mol-311 kJ/mol-11 kJ/mol
The bond enthalpies for six selected chemical bonds are shown below.Bond Bond enthalpyΔH°298 (kJ/mol)H―H 436C―H 413C=O 532N―H 335O―H 499O=O 495For a reaction in which 2 moles of H2(g) reacts with 1 mole of O2(g) to form 2 moles of H2O(g), what is the heat of the reaction?A.1367 kJB.369 kJC.−629 kJD.−1996 kJ
Given the following bond dissociation energies, calculated the enthalpy of the following reaction.CH4 + 2F2 → CF4 + 2H2Hint: You might need to draw Lewis Dot Structures for each of these before you can count the bonds on the reactant and product sides.C-F 450 kJ/molC-H 410 kJ/molF-F 158 kJ/molH-H 436 kJ/molGroup of answer choices318 kJ-716 kJ-318 kJ716 kJ
Find the enthalpy of formation of acetylene (C2H2): 2C+H2 C2H2If the enthalpy of combustion of C, H2 and C2H2 are -400kj.mol-1, -300kj.mol-1 and-1300kj.mol-1?
Calculate the heat of reaction ΔH for the following reaction:H2(g)+ Cl2(g)→2HCl(g)You can find a table of bond energies by using the Data button on the ALEKS toolbar.Round your answer to the nearest /kJmol.
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.