Question

The major industrial source of hydrogen gas is by the following reaction: CH4(g) + H2O(g) ------>...

The major industrial source of hydrogen gas is by the following reaction:

CH4(g) + H2O(g) ------> CO(g) + 3 H2(g)

Use bond energies to predict deltaH for this reaction.

So I used bond energy chart:

CH4(g): 4mol C-H= 4*413kJ/mol

H2O(g): 2mol H-O = 2*467kJ/mol

3 H2(g): 3mol H-H = 3*432kJ/mol

CO(g): 1mol C-O = 1*358kJ/mol

And I got the answer as 1290kJ.... but it is wrong because apparently for CO(g) the bond has to be a triple bond...so the energy for C triple bond O would be 1072kJ.

Overall answer is 218kJ.

How do I figure out that CO(g) is a triple bond not single bond...?

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Homework Answers

Answer #1

CH4(g) + H2O(g) ------> CO(g) + 3 H2(g)

CH4(g): 4mol C-H= 4*413kJ/mol

H2O(g): 2mol H-O = 2*467kJ/mol

3 H2(g): 3mol H-H = 3*432kJ/mol

Bond energy of CO= 1072kJ/mol

dHrxn = dH products - dH reactants

dH rxn = (3*432)+1072 - (4*413)-(2*467)

dH rxn = -218 kJ.mol

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