What conditions will favour a high concentration of SO3 (g) for the reaction is
SO2(g) + 1/2O2(g) = SO3(g) + 96kJ
There are several conditions that can favor a high concentration of SO3 in the reaction:
1. Decreased temperature: According to Le Chatelier's principle, decreasing the temperature will shift the reaction towards the side with fewer moles of gas. Since SO2 and O2 have a total of 1.5 moles of gas while SO3 has only 1 mole of gas, a decrease in temperature will favor the formation of SO3.
2. Increased pressure: Higher pressures will also favor the side with fewer moles of gas. Increasing the pressure will push the equilibrium towards the side of the reaction with a smaller number of moles of gas. Therefore, increasing the pressure will lead to a higher concentration of SO3.
3. Use of a catalyst: The use of a catalyst will increase the rate of reaction, allowing the system to reach equilibrium faster. This can result in a higher concentration of SO3 since the reaction will have more time to proceed towards completion.
4. Removal of product: By continuously removing SO3 from the reaction mixture, you can shift the equilibrium towards the product side. This can be done by using a condenser to condense the SO3 and remove it from the reactor.
5. Stoichiometric excess of reactants: By using an excess of SO2 and O2, the reaction can be driven towards the formation of SO3. This ensures that there are enough reactants available to react and form the desired product.
6. Optimized reaction conditions: Fine-tuning the temperature, pressure, and reactant concentrations can lead to optimal conditions for generating a high concentration of SO3. This can include finding the temperature and pressure ranges that favor the forward reaction while considering the energy requirements of the reaction.
It should be noted that the reaction is exothermic, meaning it releases heat (96 kJ). Therefore, while these conditions favor the formation of SO3, balancing the reaction with energy considerations is also essential.