Question

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.

Answer 1

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.

Answer 2

The enthalpy for the formation of carbon dioxide has been -626 kJ/mol.

$\Delta$H has been the energy required for the breaking of the bonds in the dissociation reaction, and the energy for the formation of bond.

Given, $\Delta$H H-O bond = 459 kJ/mol

$\Delta$H for H-H bond = 432 kJ/mol

$\Delta$H for C=O bond = 799 kJ/mol

$\Delta$H = Energy for breaking bond - energy for bond formation

$\Delta$H = (4 times H-O bond) - (2 time H-H bond + 2 times C=O bond formation)

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

$\Delta$H = 1,836 - (1,598 + 864) kJ/mol

$\Delta$H = 1,836 - 2,462 kJ/mol

$\Delta$H = -626 kJ/mol

The enthalpy for the formation of carbon dioxide has been -626 kJ/mol.

For more information about the production of hydrogen, refer to the link:

https://brainly.com/question/19790865