Step 2 is a reversible reaction so the conditions can be altered to get the right balance of equilibrium
2 SO2 + O2 ⇌ 2 SO3
TEMPERATURE - Oxidising sulfure dioxide to form sulfur trioxide is an exothermic reaction, so to get more product the temperature should be reduced which would shift it to the right, but this would slow downt he reaction. a compromise of 450' is used
PRESSURE - There are two moles of product compared to three moles of reactant. so to get mroe product pressure should increase to move it towards the right. but increasing pressure is expensive and equilibrium is already on the right so its not necessary - meaningatmposheric pressure (1 atmosphere) is used
CATALYST - to increase the rate of the reaction a catalyst of vanadium pentoxide is used which doesnt effect the equilibrium
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