ThermochemistryHard

Question

Calculate the enthalpy of the following homogeneous gaseous reaction

CH3COCH3 + 2O2 → CH3COOH + CO2 + H2O

from the following data.

Bond energies (kJ/mol): C−H = 414; C−C = 348; C=O = 580; C−O = 354; O=O = 610; O−H = 462;

Magnitude of resonance energies (kJ/mol): COOH =118; CO2 = 140.

Options

A.348 kJ
B.168 kJ
C.−168 kJ
D.−348 kJ

Solution

$\Delta H_{\text{Required}} = \lbrack 6 \times 414 + 2 \times 348 + 580 + 2 \times 610\rbrack $$$ - \lbrack 3 \times 414 + 348 + 580 + 354 + 462 + 118 + 2 \times 580 + 140 + 2 \times 462\rbrack = - 348\text{ kJ}$$

Create a free account to view solution

View Solution Free
Topic: Thermochemistry·Practice all Thermochemistry questions

More Thermochemistry Questions

The standard enthalpy of formation of NH3 is - 46.0 kJ mol-1. If the enthalpy of formation of H2 from its atoms is - 436...Enthalpies of solution of BaCl2(s) and BaCl2·2H2O(s) are −20.6 kJ/mol and 8.8 kJ/mol, respectively. ΔH hydration of BaCl...Combustion of glucose takes place according to the equation :C6H12O6 + 6O2 → 6CO2 + 6H2O, ᐃH = - 72 kcalThe ...Which of the following reaction(s) is/are endothermic?...The heat of reaction for : C10H8(s) + 12O2(g) → 10CO2(g) + 4H2O(l) at constant volume is 1228.2 kcal at 25oC. The ...