Question

How would I go about doing this?

839 kJ/mol C ≡ C # of bonds ______ (product / reactant) side Energy:_____ 495 kJ/mo O = O # of bonds ______ (product / reactant) side Energy:_____ 413 kJ/mo C—H # of bonds ______ (product / reactant) side Energy:_____ 358 kJ/mo C—O # of bonds ______ (product / reactant) side Energy:_____ 467 kJ/mo H—O # of bonds ______ (product / reactant) side Energy:_____
Add the energies on the reactant side __________ kJ/mol
Add the energies on the product side __________ kJ/mol
This reaction is (exothermic / endothermic)
The reaction (produces / absorbs) __________ kJ when ____ moles of acetylene (C2H2) reacts.

Answer 1

Based on the values of bond energies given, the reaction is endothermic and absorbs 20 kJ of heat when 2 moles of acetylene reacts.

What is the energy change in the combustion of acetylene, C2H2?

The equation of the combustion of acetylene sis given below:

2 C2H2 + 5 O2 -----> 4 CO2 + 2 H2O

• Heat change, ΔH = Sum ΔH of bonds broken - sum of ΔH of bonds formed.

Sum of ΔH bonds broken:

2 × C≡C + 2(2 × C—H) = 2 × 839 + 4 × 413 = 3330 kJ

5 × (2 × O = O) = 10 × 495 = 4950 kJ

Sum of ΔH bonds broken = 8280 kJ

Sum of ΔH of bonds formed:

Energy of C=O is 799 kJ

4 × 2 × C=O = 8 × 799 = 6392 kJ

Energy of H-O bond is 467kJ

2 × 2 × H-O = 2 × 2 × 467 = 1868 kJ

Sum of ΔH of bonds formed = 8260 kJ

Heat change, ΔH = 8280 -8260 kJ

Heat change, ΔH = 20 kJ

Therefore, based on the bond energies given, the reaction is endothermic and absorbs 20 kJ of heat when 2 moles of acetylene reacts.

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