1. 839 kJ/mol C=C # of bonds is 2 it’s reactant, Energy: ____
2. 495 kJ/mo. 0=0. # of bonds is 5 it’s reactant, Energy: ______
3. 413 kJ/mo. С—Н. # of bonds is 4 it’s reactant, Energy:____
4. 745 kJ/mo. C=0. # of bonds is 8 it’s Product, Energy: ______
5. 467 kJ/mo. Н-О. # of bonds is 4 its product, Energy: _______
This is what I think it is, is it correct?
Energy: 1578
Energy: N1
Energy: N2
Energy: N3
Energy: N9
Also make sure to:
Add the energies on the reactant side ___ kJ/mol
Add the energies on the product side ____ KJ/mol
This reaction is (exothermic or endothermic)
The reaction (produces or absorbs) kJ when 2 moles of acetylene (C2H2) reacts.
Based on the information provided, the correct energies and information can be determined as follows:
1. 839 kJ/mol C=C: This is the energy of one C=C bond in the reactant side. We have 2 C=C bonds, so the total energy on the reactant side is 2 * 839 = 1678 kJ/mol.
2. 495 kJ/mol O=O: This is the energy of one O=O bond in the reactant side. We have 5 O=O bonds, so the total energy on the reactant side is 5 * 495 = 2475 kJ/mol.
3. 413 kJ/mol C-H: This is the energy of one C-H bond in the reactant side. We have 4 C-H bonds, so the total energy on the reactant side is 4 * 413 = 1652 kJ/mol.
4. 745 kJ/mol C=O: This is the energy of one C=O bond in the product side. We have 8 C=O bonds, so the total energy on the product side is 8 * 745 = 5960 kJ/mol.
5. 467 kJ/mol H-O: This is the energy of one H-O bond in the product side. We have 4 H-O bonds, so the total energy on the product side is 4 * 467 = 1868 kJ/mol.
The reaction produces 1678 kJ/mol on the reactant side and absorbs 7828 kJ/mol on the product side.
Since the reaction absorbs more energy than it produces, it is an endothermic reaction.
Please note that the energies provided are assumed values and may vary in actual chemical reactions.