For a reaction if Kp>Kc , the forward reaction is favoured by
Correct answer: C. Low Pressure
- A. High Temperature
- B. Low Temperature
- C. Low Pressure
- D. High Pressure
Explanation
According to the relation Kp = Kc(RT)Δn, if Kp > Kc, then Δn > 0, meaning the number of moles of gas increases on the product side of the reaction. To favor the forward reaction under these conditions, one would decrease the pressure. Decreasing pressure shifts the equilibrium towards the side with more moles of gas-in this case, the product side. Temperature changes are not directly related to this comparison, hence both high and low temperature options are incorrect. High pressure, which favors the side with fewer moles, is also incorrect in this context.
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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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