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Elden [556K]
4 years ago
14

Hydrogen, a potential future fuel, can be produced from carbon (from coal) and steam by the following reaction: C(s)+2H2O(g)→2H2

(g)+CO2(g) Note that the average bond energy for the breaking of a bond in CO2 is 799 kJ/mol.
Chemistry
1 answer:
madam [21]4 years ago
5 0

The question is incomplete , complete question is:

Hydrogen, a potential future fuel, can be produced from carbon (from coal) and steam by the following reaction:

C(s)+ 2 H_2O(g)\rightarrow 2H_2(g)+CO_2(g).\Delta H=?

Note that the average bond energy for the breaking of a bond in CO2 is 799 kJ/mol. Use average bond energies to calculate ΔH of reaction for this reaction.

Answer:

The ΔH of the reaction is -626 kJ/mol.

Explanation:

C(s)+ 2 H_2O(g)\rightarrow 2H_2(g)+CO_2(g).\Delta H=?

We are given with:

\Delta H_{H-O}=459 kJ/mol

\Delta H_{H-H}=432 kJ/mol

\Delta H_{C=O}=799 kJ/mol

ΔH =  (Energies required to break bonds on reactant side) - (Energies released on formation of bonds on product side)

\Delta H=(4\times \Delta H_{O-H})-(2\times \Delta H_{H-H}+2\times\Delta H_{C=O})

=(4\times 459 kJ/mol)-(2\times 432 kJ/mol+2\times 799 kJ/mol

\Delta H=-626 kJ/mol

The ΔH of the reaction is -626 kJ/mol.

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Note: Kindly find an attached image below for the part of the solution to this question

Sources: The image was researched from Course hero platform

Explanation:

Solution

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It helps in determination of multiplicity of an individual proton or individual types of proton which are available in the molecule.

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