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 1200 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 1200 K, Kp > 1
- D. At 300 K, the products will be favoured more than reactants at equilibrium
Explanation
The solution for this question is given below:
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About Chemical Equilibrium
Reversible reactions reach dynamic equilibrium when forward and reverse rates become equal, and Le Chatelier's principle predicts the effect of changing concentration, pressure or temperature. The chapter also covers solubility product, the common ion effect, buffer action and the conditions used in Haber's process, with equilibrium shifts distinguished from changes in the equilibrium constant.
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