Answer:
ΔHrxn = - 3294.8 KJ/mol
Explanation:
H - H H - O - H
H - H + O = O → H - O - H
broken bond:
⇒ 2 bond H - H + 1 bond O = O
bond formed:
⇒ 4 bond H - O
bond energies:
∴ H - H: 436.4 KJ/mol
∴ O = O: 494 KJ/mol
∴ H - O: 482 KJ/mol
broken bond:
⇒ bond energie = 2(436.4) + 494 = 1366.8 KJ/mol
bond formed:
⇒ bond energie = 4(- 482) = - 1928 KJ/mol
⇒ ΔHrxn = - 1928 KJ/mol - (1366.8 KJ/mol)
⇒ ΔHrxn = - 3294.8 KJ/mol
By using the average bond energies, the [tex]\Delta H[/tex] for the chemical reaction of hydrogen gas ([tex]H_2[/tex]) and oxygen gas ([tex]O_2[/tex]) react chemically to form water ([tex]H_2O[/tex]) is 402 kJ.
Bond energy can be defined as the amount of energy that is required to break one (1) mole of a particular chemical bond and it is measured in kJ/mol.
Hydrogen gas ([tex]H_2[/tex]) and oxygen gas ([tex]O_2[/tex]) react chemically to form water ([tex]H_2O[/tex]) as shown in this balanced chemical equation:
[tex]2H_2 + O_2 --->2H_2O[/tex]
The following bonds are formed from the above chemical reaction:
[tex]H-H = 436 \;kJ/mol[/tex]
[tex]O-O = 494 \;kJ/mol[/tex]
[tex]H-O = 482 \;kJ/mol[/tex]
Energy in:
[tex]2(436) + 494 = 1,366\;kJ/mol[/tex]
Energy out:
[tex]2(482) = 964 kJ/mol[/tex]
Now, we can calculate the [tex]\Delta H[/tex] for the chemical reaction by using this formula:
[tex]\Delta H = E_{in} - E_{out}\\\\\Delta H = 1366-964\\\\\Delta H =402 \;kJ[/tex]
Change in energy = 402 kJ.
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