The standard enthalpy and entropy changes for the reaction in equilibrium for the forward reaction are given below: CO (g) + H2O (g) <-> CO2 (g) + H2 (g)∆Hº 300K = - 41.16 kJ mol-1∆Sº 300K = - 4.24 x 10^-2 kJ mol-1∆Hº 1200K = - 32.93 kJ mol-1Then, the incorrect statement is :
Correct answer: C. At 300 K, Kp > 1
- A. The reaction proceeds in the forward direction at 300 K
- B. At 1200 K, reaction proceeds in the reverse direction
- C. At 300 K, Kp > 1
- D. At 300 K, the products will be favoured more than reactants at equilibrium
Explanation
This is the following solution: kp is less than one, reaction is non spontaneous for sponataneous reactions kp is greater than one
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About Enthalpy
Enthalpy is the heat content of a system measured at constant pressure, and its change indicates whether a reaction or physical process is endothermic or exothermic. The topic covers state functions, enthalpy diagrams, standard enthalpy of formation, combustion and neutralisation, and the relationship between ΔH and internal energy change.
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