Water gas (a mixture of carbon monoxide and hydrogen) is prepared by passing steam over red-hot coke: c(s) + h2o(g)
→co(g) + h2(g)for many years, water gas was used as a fuel in industry and for domestic cooking. compare the heat produced by the complete combustion of 1 mole of methane (ch4) with a mole of water gas (0.50 mole h2 and 0.50 mole co) under standard conditions. (assume liquid water is formed.) what is the difference between the two values? (in kj/mol)

The answer to this is -605.5 KJ/mol

Explanation:

The process of passing steam over red-hot will result in:

C(s) + H2O(g)  →CO(g) + H2(g);

Complete combustion of CH₄, H₂  and CO results in

CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)   ΔH = -890 kJ/mol

Therefore energy needed to produce C02 is,

CO(g) + 1/2O2(g) → CO2(g)  ΔH = -283 kJ/mol

while that of H20;

H2(g) + 1/2O2(g) → H2O(l)  ΔH = -286 kJ/mol

from the equations above; heat combustion for H20 = -286KJ/mol;

CO2 = -283KJ/mol

CH4 = -890KJ/mol...

Get the average energy between the combustion of H20 and CO2 to determine the value of water gas used for many years

(-283 -286)KJ/mol /2 = 284.5KJ/mol

Assumption of liquid water;

Difference between the two values is:

-890kJ/mol - (-284.5kJ/mol) = -605.5 kJ/mol

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