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I assume this is the reaction you are talking about:
CH4 + H2O (g) --> CO(g) + 3H2(g)
From thermodynamics you can approximate the standard heat of reaction Hrxn with Hess' Law. This is the sum of the heats of formations of the products minus the sum of the heats of formations of the reactants in their stoichemtric ratios.
Hrxn = SUM [(3)*Hf (H2)+(1)*Hf(CO)] - SUM [(1)*Hf (CH4) + (1)*Hf(H2O (g))]
Looking up these values in a Chemical Engineering Handbook or textbook we can substitue and find the heat of reaction.
Hrxn = SUM [(3)*(0 kJ/mol) + (1)*(-110.52 kJ/mol)] - SUM [(1)*(-74.85 kJ/mol) +
(1)*(-241.83 kJ/mol)]
= -110.52 - (-316.68) kJ/mol
= + 206.16 kJ/mol, therefore the reaction is endothermic
Remember standard heats of formation of elements, as hydrogen in this case, are zero.
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