Question

Given the bond energies below, calculate an estimate for ΔH (kJ) for the reaction: 2CO(g) + O2(g) –> 2CO2(g) Bond energy (kJ/mol): C-O, 360; C=O, 799; CO(triple bond), 1071; O2, 498

Answer 1

To estimate ΔH (kJ) for the reaction: 2CO(g) + O2(g) → 2CO2(g), we need to calculate the energy required to break the bonds in the reactants side and the energy released by forming the bonds in the products side. Subtracting the energy required from the energy released gives us the change in enthalpy.

Step-by-step explanation:

To calculate an estimate for ΔH (kJ) for the reaction: 2CO(g) + O2(g) → 2CO2(g), we need to use the bond energies provided. First, we calculate the energy required to break the bonds in the reactants side: 2 C-O bonds and 2 C=O bonds. The sum of these bond energies is 2 x 360 kJ/mol + 2 x 799 kJ/mol = 2718 kJ/mol. Then, we calculate the energy released by forming the bonds in the products side: 4 CO2 bonds. The sum of these bond energies is 4 x 1071 kJ/mol = 4284 kJ/mol. Finally, we calculate the change in enthalpy by subtracting the energy required from the energy released: ΔH = energy released - energy required = 4284 kJ/mol - 2718 kJ/mol = 1566 kJ/mol.