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Use the reaction equation and bond energies to answer the question.2H20 - 2H2 + 02H-O: 467 kJ/molH-H: 432 kJ/molO=0: 495 kJ/molWhat is the total energy of the reaction? Is this an endothermic or exothermic reaction? okay

Use the reaction equation and bond energies to answer the question2H20 2H2 02HO 467 kJmolHH 432 kJmolO0 495 kJmolWhat is the total energy of the reaction Is thi class=

Respuesta :

Answer:

The total energy of the reaction is 2,237kJ/mol.

The reaction is endothermic.

Explanation:

To calculate the total energy of the reaction, it is necessary to subtract each bond energy in the reaction:

- Bonds broken (to the left of the arrow):

[tex]\begin{gathered} \\ 2H_2O:2*\left(467kJ/mol+467kJ/mol\right)=1868kJ \\ 2H_2:2*(432kJ/mol)=864kJ/mol\text{ } \\ \\ \end{gathered}[/tex]

Total broken bonds: 2,732kJ/mol

- Bonds made (to the right of the arrow):

[tex]O_2:495kJ/mol[/tex]

Total made bonds: 495kJ/mol

Finally, we have to subtract the total broken bonds minus total made bonds:

[tex]\begin{gathered} \text{ Total bond energy: 2,732kJ/mol-495kJ/mol} \\ \text{ Total bond energy: 2,237kJ/mol} \end{gathered}[/tex]

So, the total energy of the reaction is 2,237kJ/mol, and the positive sign means that the reaction is endothermic.

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