Generating hydrogen gas using the least amount of energy possible is very desirable. One proposed scheme is the catalyzed decomposition of formic acid, HCO₂H. [S. Ott, Science, Vol. 333, pp. 1714–1715, 2011.]

A particularly interesting aspect of this reaction is that it can be run in reverse and so serve as a way of storing hydrogen. Calculate the equilibrium constant (at 298 K) for the decomposition reaction using thermodynamic data. Is the decomposition reaction product-favored at equilibrium at 298 K? (For HCO₂H(g), Δ_fH° = −378.6 kJ/mol and S° = 248.70 J/K·mol.)

Transcribed Image Text:

HCO₂H(g) → CO₂(g) + H₂(g)