Reversible reactions are known to be subject to equilibrium limitations. These l

Question

Reversible reactions are known to be subject to equilibrium limitations. These limitations (equilibrium conversion); however, might depend on the type of reactor and the operating conditions. The plot below shows the effect of adding inerts (theta 1 = 1 C1 degree/CA degree) on the equilibrium limitations for a constant volume batch reactor and those of an (equivalent) tubular (with a negligible pressure drop) reactor, for the elementary gas-phase reaction. (a) Can you explain why flow reactors seem to be less restricted by equilibrium limitations than constant volume batch reactors?

Explanation / Answer

Adding inert gas at constant volume decreases the partial pressure of the reactant A and product B. Since, for every mole of A, there are 2 moles of B is produced. Therefore, the equilibrium shifts to the left, that is reversible reaction is favoured and the equilibrium concentration of A, CA is increased by adding inert gas into the system.

The reason why in the flow reactors this restriction is less affected is the pressure change is negligible. Since the pressure change is negligible, the equilibrium shift is not as much as it is in constant volume batch reactor.

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