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Travka [436]
3 years ago
6

Using bond energies, estimate the enthalpy of reaction for the following chemical reaction. CH4(g) + 4 F2(g) → CF4(g) + 4 HF(g)

ΔHrxn = ?
Chemistry
1 answer:
MrRa [10]3 years ago
7 0

Answer:

\mathbf{ \Delta H_{rxn} =   -1936 \ kJ/mol}}

Explanation:

The equation for the reaction is given as:

\mathbf{    CH_{4(g)} + 4 F_{2(g)} \to CF_{4(g)} + 4 HF_{(g) }}

At standard conditions; the bond energies are as follows;

Bond       Bond Energies (kJ/mol)

C-H           413

F-F            155

C-F            485

H-F            567

\mathbf{\Delta \ H_{rxn} =  \sum \Delta H ( reactant) - \sum \Delta H (product)}

\mathbf{\Delta \ H_{rxn} =  \sum [\Delta H \ 4( C-H) + \Delta H \ 4(F-F) ]- \sum[ \Delta H \ 4( C-F)+\Delta H \ 4( H-F)]   (product)}

\mathbf{\Delta \ H_{rxn} = \sum{ \Delta \ H  (4*413) + \Delta  \ H (4*155) - \Delta \ H  (4(485)) + \Delta H (4(567) }}

\mathbf{ \Delta H_{rxn} = \sum  ({ (1652 + 620) - (1940 + 2268)})}

\mathbf{ \Delta H_{rxn} = \sum  ({2272- 4208})}

\mathbf{ \Delta H_{rxn} =   -1936 \ kJ/mol}}

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Here's what I find.

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