The equation for this equilibrium reaction is C2H6—> C2H6 + H2. The forward reaction takes in heat energy and is endothermic. A manufacturer produces large quantities of propene using this equilibrium reaction. Suggest, with explanations, suitable conditions that the manufacturer could use to maximise the yield and rate of production of propene from propane – 9032

One thought on “The equation for this equilibrium reaction is C2H6—> C2H6 + H2. The forward reaction takes in heat energy and is endothermic. A manufacturer produces large quantities of propene using this equilibrium reaction. Suggest, with explanations, suitable conditions that the manufacturer could use to maximise the yield and rate of production of propene from propane – 9032”

1. Using a catalyst like platinum speeds up both the forward and backward reactions. This means equilibrium is reached faster, but the catalyst does not affect the overall yield of the product.
   A higher temperature increases the rate of reaction because particles move faster and collide more often. It also shifts the equilibrium to the right-hand side, increasing the yield. A temperature between 200°C and 600°C would be suitable. However, very high temperatures use more energy, which makes the process more expensive.
   Since there are fewer molecules on the left side of the reaction than the right, using a low pressure shifts the equilibrium to the right, which increases the yield. But lower pressure also slows the rate of reaction. High pressure would increase the rate but reduce the yield, so the pressure used is a compromise between rate and yield.

   Reply