Answer: 12033 kJ of heat produced per kg of [tex]CO_2[/tex] formed during the combustion of benzene
Explanation:
The balanced chemical equation for combustion of benzene is :
[tex]2C_6H_6(l)+15O_2(g)\rightarrow 12CO_2(g)+6H_2O(g)[/tex] [tex]\Delta H°rxn[/tex] = -6278 kJ
Exothermic reactions are defined as the reactions in which energy of the product is lesser than the energy of the reactants. The total energy is released in the form of heat and [tex]\Delta H[/tex] for the reaction comes out to be negative.
[tex]\text{Moles of }CO_2=\frac{\text{given mass}}{\text{Molar Mass}}=\frac{1000g}{44g/mol}=23mol[/tex] (1kg=1000g)
According to stoichiometry :
12 moles of [tex]CO_2[/tex] on combustion produce heat = 6278 kJ
Thus 23 mole of [tex]CO_2[/tex] on combustion produce heat =[tex]\frac{6278}{12}\times 23=12033kJ[/tex]
Thus 12033 kJ of heat produced per kg of [tex]CO_2[/tex] formed during the combustion of benzene
1.189 × 10⁴ kJ of heat are produced per kg of CO₂ formed during the combustion of benzene.
Let's consider the following thermochemical equation for the combustion of benzene.
2 C₆H₆(l) + 15 O₂(g) → 12 CO₂(g) + 6 H₂O(g) ΔH°rxn = -6278 kJ
First, we will convert 1 kg (1000 g) of CO₂ to moles using its molar mass (44.01 g/mol).
[tex]1000 g \times \frac{1mol}{44.01g} = 22.72 mol[/tex]
Considering the standard enthalpy of the reaction given in the thermochemical equation, 6278 kJ of heat are released when 12 moles of CO₂ are produced. The heat released when 22.72 moles of CO₂ are produced is:
[tex]\frac{-6278kJ}{12mol} \times 22.72 mol = -1.189 \times 10^{4} kJ[/tex]
1.189 × 10⁴ kJ of heat are produced per kg of CO₂ formed during the combustion of benzene.
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