The most important commercial process for generating hydrogen
gas is the water-gas shift reaction:
CH4(g) + H2O(g) → CO(g) +
3H2(g)
Use tabulated thermodynamic data to find ΔG° for this reaction at
the standard temperature of 25°C.
1.423×102 kJ
Calculate ΔG°1000 for this process when it occurs at
1000 K
.
CH4(g) + H2O(g) → CO(g) + 3H2(g)
from standard data
DHrxn = (DH0fCO + 3*DH0fH2) - (1*DH0fCH4+1*DH0fH2O)
= (-110.5 + 3*0) - (-74.8 -241.8)
= 206.1 kj
DSrxn = (S0fCO + 3*S0fH2) - (1*S0fCH4+1*S0fH2O)
= (197.9 +3*130.59) - (186.27+188.72)
= 214.68 j/mol.k
DG = DH - TDS
at T = 25 C = 298 k
DG = 209.1 - (298*214.68*10^-3) = 145.12 kj
at T = 1000 k
DG = 209.1 - (1000*214.68*10^-3) = -5.58 kj
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