The standard enthalpy and entropy changes for the reaction in equilibrium for the forward direction are given below:
CO(g)+H_(2)O(g)?CO_(2)(g)+H_(2)(g) \Delta H_(300K)^(o)=-41.16kJmol^(-1) \Delta S_(300K)^(o)=-4.24\times 10^(-2)kJmol^(-1) \Delta H_(1200K)^(o)=-32.93kJmol^(-1) \Delta S_(1200K)^(o)=-2.96\times 10^(-2)kJmol^(-1)
Calculate
K_(P)
at each temperature and predict the direction of reaction at
300K
and
1200K
, when
P_(CO)=P_(CO_(2))=P_(H_(2))=P_(H_(2)O)=1atm
at initial state.

Question

The standard enthalpy and entropy changes for the reaction in equilibrium for the forward direction are given below:

CO(g)+H_(2)O(g)?CO_(2)(g)+H_(2)(g)
\Delta H_(300K)^(o)=-41.16kJmol^(-1)
\Delta S_(300K)^(o)=-4.24\times 10^(-2)kJmol^(-1)
\Delta H_(1200K)^(o)=-32.93kJmol^(-1)
\Delta S_(1200K)^(o)=-2.96\times 10^(-2)kJmol^(-1)

Calculate

K_(P)

at each temperature and predict the direction of reaction at

300K

and

1200K

, when

P_(CO)=P_(CO_(2))=P_(H_(2))=P_(H_(2)O)=1atm

at initial state.

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