The reaction is carried out at a pressure of 200 atmospheres. Explain what effect a pressure higher than 200 atmospheres would have on the rate of attainment of equilibrium and on the equilibrium yield of ammonia. – 9025

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1. When pressure is increased, the particles are forced closer together, which makes collisions between reacting particles more frequent, so the reaction happens faster. This means that equilibrium is reached more quickly.

   Also, if the forward reaction produces fewer gas molecules than the backward reaction, the system will respond to the increase in pressure by shifting the equilibrium to the side with fewer molecules, which is the right side or the products side.

   As a result, more products are formed, so the equilibrium yield increases.

   So, increasing pressure helps to:
   • reach equilibrium faster,
   • increase the amount of product formed,
   • and shift the equilibrium position to the right side (products),
   • because the number of molecules is lower on that side

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