The significance of ΔG° (gibbs energy change) is that it is positive , so reaction is non-spontaneous .
Given , the reaction is ,
CH3OH (g) ⇔ CO (g) + 2H2 (g)
(a)ΔH°rxn = -110.54 + 2×0 - (-201.08) kj = 90.54kj
ΔS°rxn = 197.9 +(2×130.59) - ( 2×239.7) J/K = -20.32J/K
(b) ΔG°rxn (at 28°C) = ΔH° - TΔS°
= 90.54 - [301× (-20.32×10^-3)]KJ
ΔG°rxn (at 28°C) = 96.66kj
ΔG°rxn (at 128°C) = 90.54 - [401×(-20.32×10^-3)]
ΔG°rxn (at 128°C) =98.69 KJ
ΔG°rxn(at 228°C) = 90.54 - [ 501×(-20.32×10^-3)]
ΔG°rxn(at 228°C) = 100.72KJ
(C) Significance of ΔG°rxn :
if ΔG° is positive , then the reaction is non-spontaneous .
if ΔG° is negative , then the reaction is spontaneous .
in these three temperature ΔG° is positive , so the reaction is non- spontaneous .
Also in increase in temperature ΔG°rxn increases i.e. rate of forward reaction decreases . so increase in temperature , the rate of reverse reaction increases .
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Question :
one reaction used to produce small quantities of pure H2 is
CH3OH(g)⇔CO(g) + 2H2 (g)
(a) determine ΔH°rxn and ΔS°rxn for the reaction at 298K .
(b) assuming that these values are relatively independent of temperature , calculate ΔG°rxn at 28°C , 128°C, 228°C .
(c) what is the significance of the different ΔG°rxn ?
