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https://1drv.ms/w/s!AnPqX9obAro6g2SGlk27MXKDWiP3?e=mlmZ0nWhen calculating the sum of the bond energies, each bond in the reaction must be accounted for. For example, CH4 is a reagent with a coefficient of 1 in the reaction. There are four C−H bonds in methane and one methane molecule per reaction, for a total of four C−H bonds on the reactant side. All four bonds must be accounted for when finding the sum of the bond energies for the reactants.Calculate the heat of reaction using the average bond dissociation energies given in the introduction and your answer to Part B for the reactionCH4 + 2O2 → CO2 + 2H2OExpress your answer in kilojoules per mole to three significant figures.

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Answer :

Answer:

[tex]969\text{kJ/mol}[/tex]

Explanations:

Given the reaction between methane and oxygen expressed as:

[tex]CH_4+2O_2\rightarrow CO_2+2H_2O[/tex]

The given energy of the bonds from the given table are:

C—H = 413 kJ/mol

O₂ = O—O = 498kJ/mol

H₂O = O—H = 467kJ/mol

CO₂ = C=O = 745 kJ/mol

The dissociation energy is expressed according to the formula;

[tex]Q=E_f-E_b[/tex]

where:

Ef is the energy of bonds are formed during the reaction, kJ/mol;

Eb is the energy of bonds are broken during the reaction, kJ/mol

[tex]\begin{gathered} Q=\lbrack(4C-H)+2O-O\rbrack-\lbrack2(O-H)+C=O\rbrack \\ Q=\lbrack4(413)+2(498)\rbrack-\lbrack2(467)+745\rbrack \\ Q=(1652+996)-(934+745) \\ Q=2648-1679 \\ Q=969\text{kJ/mol} \end{gathered}[/tex]

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