The following data give the energy needed to break the indicated bond. In the case of multiple bonds the energy applies to breaking the multiple bond completely:Bond Bond Dissociation EnergykJ/molBond Bond Dissociation EnergykJ/molC-H 413 C=O 745*C-C 347 C=C 614C-N 305 C≡C 839C-O 358 O=O 495O-H 463 N≡N 946 *C=O in carbon dioxide 804 kJ/molCalculate the energy required to dissociate all atoms, that is break all chemical bonds, in 1.00 mole of ethene, CH2CH2.Question 2Select one:a.2266 kJb.1038 kJc.2880 kJd.1027 kJe.- 2266 kJ

The molecular structure of ethene (CH2CH2) consists of 4 C-H bonds, 1 C-C bond, and 1 C=C bond.

To calculate the total energy required to break all these bonds in 1 mole of ethene, we need to add up the bond dissociation energies for each type of bond, multiplied by the number of each bond in the molecule.

From the data given:

• Energy to break C-H bond = 413 kJ/mol. There are 4 C-H bonds in ethene, so total energy = 4 * 413 = 1652 kJ/mol
• Energy to break C-C bond = 347 kJ/mol. There is 1 C-C bond in ethene, so total energy = 1 * 347 = 347 kJ/mol
• Energy to break C=C bond = 614 kJ/mol. There is 1 C=C bond in ethene, so total energy = 1 * 614 = 614 kJ/mol

Adding these up, the total energy required to dissociate all atoms in 1 mole of ethene = 1652 + 347 + 614 = 2613 kJ/mol

However, none of the options provided (a. 2266 kJ, b. 1038 kJ, c. 2880 kJ, d. 1027 kJ, e. - 2266 kJ) match this calculated value. Please check the question or the options again.

The molecular structure of ethene (CH2CH2) consists of 4 C-H bonds, 1 C-C bond, and 1 C=C bond.

To calculate the total energy required to break all these bonds in 1 mole of ethene, we need to add up the bond dissociation energies for each type of bond, multiplied by the number of each bond in the molecule.

From the data given:

• Energy to break C-H bond = 413 kJ/mol. There are 4 such bonds in ethene, so total energy = 4 * 413 = 1652 kJ/mol
• Energy to break C-C bond = 347 kJ/mol. There is 1 such bond in ethene, so total energy = 1 * 347 = 347 kJ/mol
• Energy to break C=C bond = 614 kJ/mol. There is 1 such bond in ethene, so total energy = 1 * 614 = 614 kJ/mol

Adding these up, the total energy required to dissociate all atoms in 1 mole of ethene = 1652 + 347 + 614 = 2613 kJ/mol

However, none of the options given match this calculation. It's possible there may be a mistake in the question or the provided options.