Using the following thermochemical equation,determine the amount of heat produced from the combustion of 24.3 g benzene (C₆H₆) .The molar mass of benzene is 78.11 g $\mathrm { mol } ^ { - 1 }$ 2C₆H₆(l) + 15O₂(g) ? 12CO₂(g) + 6H₂O(g)
D_rH° = -6278 kJ

Question

Using the following thermochemical equation,determine the amount of heat produced from the combustion of 24.3 g benzene (C₆H₆) .The molar mass of benzene is 78.11 g

\mathrm { mol } ^ { - 1 }

2C₆H₆(l) + 15O₂(g) ? 12CO₂(g) + 6H₂O(g)
D_rH° = -6278 kJ

Quizplus · Accepted Answer

The combustion of 2 moles of benzene releases -6278 kJ. First, calculate the moles of benzene in 24.3 g: 24.3 g / 78.11 g/mol = 0.311 moles. Since 2 moles release 6278 kJ, 0.311 moles will release (6278 kJ / 2) * 0.311 = 977 kJ.

Using the Following Thermochemical Equation,determine the Amount of Heat Produced mol−1\mathrm { mol } ^ { - 1 }mol−1

Using the Following Thermochemical Equation,determine the Amount of Heat Produced $\mathrm { mol } ^ { - 1 }$