Respuesta :
Missing information:
The reaction is 2O₃(g) --> 3O₂ (g)  ΔH = -300 kJ/mol
Answer:
c
Explanation:
In the molecule of ozone, 3 oxygens are bonded, and, because each one needs to share two pairs of electrons, these 2 bonds are something between a simple and a double bond.
In the reaction of the transformation of the ozone to oxygen gas, these bonds are broken, and a double bond is formed between two oxygen atoms. The sum of the energy of the broken and the formation of the bond is the enthalpy variation of the reaction.
To break a bond, energy must be added to the system, so it's an endothermic reaction and energy is positive, so the formation is exothermic and the energy is negative. Because there're 2 ozone molecules, 4 bonds will be broken, and because there are 3 oxygen molecules, 3 bonds will be formed:
4*E - 3*500 = -300
4E = -300 + 1500
4E = 1200
E = 300 kJ/mol
So, each O3 bond has 300 kJ/mol as an average energy.
Each ozone molecule has 300 kJ/mol as an average bond energy.
The reaction is
[tex]\bold { 2O_3(g) \rightarrow 3O_2 (g)\ \ \ \ \ \ \ \ \ \ \ \Delta H = -300 kJ/mol}[/tex] Â Â
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In the molecule of ozone, there 2 double bonds are present with continuous variation. Â
The enthalpy variation of the reaction is the sum of the energy of the broken and the formation of the bond. Â
Because of 2 ozone molecules, 4 bonds will be broken, and because there are 3 oxygen molecules, 3 bonds will be formed.
[tex]\bold {4\times E - 3 \times 500 = -300}\\\\\bold {4\times E = -300 + 1500}\\\\\bold {E = 300 kJ/mol}[/tex]
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Therefore, Each ozone molecule has 300 kJ/mol as an average bond energy.
To know more about average bond enthalpy,
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