calculate the heat of reaction δh for the following reaction: 2 ch₄(g) + 3 o₂(g)→2 co(g) + 4 h₂o(g) you can…

Explanation:

Step1: Identify bonds broken

In $2CH_4$, there are $8$ C - H bonds. In $3O_2$, there are $3$ O=O bonds.

Step2: Identify bonds formed

In $2CO$, there are $2$ C≡O bonds. In $4H_2O$, there are $8$ O - H bonds.

Step3: Look up bond - energies

Let's assume C - H bond energy is $E_{C - H}$, O=O bond energy is $E_{O=O}$, C≡O bond energy is $E_{C≡O}$ and O - H bond energy is $E_{O - H}$. From the bond - energy table: $E_{C - H}=413$ kJ/mol, $E_{O=O}=498$ kJ/mol, $E_{C≡O}=1072$ kJ/mol, $E_{O - H}=463$ kJ/mol.

Step4: Calculate energy of bonds broken

Energy of bonds broken $E_{broken}=8\times E_{C - H}+3\times E_{O=O}=8\times413 + 3\times498=3304+1494 = 4798$ kJ/mol.

Step5: Calculate energy of bonds formed

Energy of bonds formed $E_{formed}=2\times E_{C≡O}+8\times E_{O - H}=2\times1072+8\times463=2144 + 3704=5848$ kJ/mol.

Step6: Calculate $\Delta H$

$\Delta H=E_{broken}-E_{formed}=4798 - 5848=-1050$ kJ/mol.

Answer:

$-1050$ kJ/mol