2SO2(g]+O2(g]⇌2SO3(g] ,4 conditions by which concentration of SO3 can be increased
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To increase the concentration of SO3 in the given reaction, the following conditions can be applied:
1. Increasing the concentration of SO2: According to Le Chatelier's principle, if the concentration of one of the reactants is increased, the equilibrium will shift in the direction that decreases that concentration. Therefore, by increasing the concentration of SO2, the equilibrium will shift toward the product side, increasing the concentration of SO3.
2. Decreasing the concentration of O2: By reducing the concentration of one of the reactants, according to Le Chatelier's principle, the equilibrium will shift in the direction that compensates for that decrease. Hence, by decreasing the concentration of O2, the equilibrium will shift toward the product side, increasing the concentration of SO3.
3. Removing SO3 as it forms: If the SO3 produced in the reaction is continuously removed from the system, the equilibrium will keep shifting towards the product side to maintain the balance. By continuously removing SO3, either by capturing it or using a catalyst that effectively converts it, the concentration of SO3 will increase over time.
4. Increasing the pressure: The given reaction involves gases, and according to Le Chatelier's principle, increasing the pressure will shift the equilibrium in the direction that reduces the number of gas molecules. Since the reaction leads to a decrease in the number of gas molecules, increasing the pressure will favor the formation of more SO3, ultimately increasing its concentration.
Remember to consult your textbook or other reliable sources to ensure accuracy and to further deepen your understanding of these concepts.