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For a gaseous reaction, K(p) gt K(c). Wh...

For a gaseous reaction, `K_(p) gt K_(c)`. What will be the effect on equilibrium if pressure is increased at constant temperature? Will it affect the yields of the products?

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According to the relation `K_(p)=K_(c)(RT)^(Deltan)`, if `K_(p) gtK_(c)`, then `Deltan gt0`. The positive value of `Deltan` implies that the reaction occurs with an increase in volume in the forward direction. For such a reaction, if pressure is increased at equilibrium, then according to Le chatelier's principle the equilibrium will shift to the left and thus the yield to the product will decrease.
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