Estimate the value of the equilibrium constant at 550 K for each of the following reactions.
a) 2CO(g)+O2(g)⇌2CO2(g)
b) 2H2S(g)⇌2H2(g)+S2(g)
a) 2CO(g) + O2(g) <-------> 2CO2(g)
∆G° = ∆G°f(Products) - ∆G°f(Reactants)
= (2×∆H°f(CO2) ) - ( 2×∆H°f(CO) + ∆H°f(O2))
= ( 2× ( -394.39kJ/mol) ) - ( 2 × (-137.6kJ/mol) + 0 )
= -788.78kJ/mol + 275.2kJ/mol
= -513.6kJ/mol
∆G° = - RTlnK
-513.6kJ/mol = - 8.314(J/K mol) × 550K× 2.303logK
logK = 513.6/10.53
= 48.77
K = 5.9 × 10^48
b) 2H2S(g) <-------> 2H2(g) + S2(g)
∆G°= (∆G°f(H2) + ∆G°(S2) ) - ( 2× H2S))
= ( 0 + 0 ) - ( 2× (-21kJ/mol))
= + 42kJ/mol
∆G° = - RTlnK
42kJ/mol = - ( 8.314 × 550K × 2.303 × logK)
logK =-( 42/10.53)
= -3.99
K = 1.02×10^-4
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