Question

In lecture, you observed (or will observe) the following system, at equilibrium, in a sealed tube. NO(g) + NO2 (g) ⇌ N2O3 (g) Kc (25 C) = 0.55 Suppose you wanted to use this reaction to synthesize a large amount of N2O3 . Unfortunately, the magnitude of the equilibrium constant at 25 C is relatively small, and as a result, there is not enough N2O3 once equilibrium is established.

Describe three different experimental approachesthat you could use to increase the yield of N2O3 from thisreaction

Answer 1

One of the things that could be done to increase the yield is to play with temperature values until optimal is achieved, this is due to the reaction is exothermic, and as the temperature is decreased, le chatelier principle comes in hand shifting equilibrium to products. However, the rate will decrease, so that's why the optimal must be found.

Another approach might be to add more reactants, so that the equilibrium will be shifted to producing more N₂O₃.

Another approach will be to increase pressure, and hence, reduce volume, which will make the equilibrium try to compensate and make more product.