Equilibrium systems that include gas phases are also affected by Le Chatelier\'s
ID: 964076 • Letter: E
Question
Equilibrium systems that include gas phases are also affected by Le Chatelier's principle. One difference is the effect of pressure. If the total pressure of the system is increased, then the system will shift toward the reaction side that has fewer moles of gas. Of course, if the total pressure of the system is decreased, then the system will shift toward the reaction side that has more moles of gas. For the equilibrium system below, state which way the system is expected to shift to offset the given changes. Then explain what happens to the partial pressure (or concentration) of SO^2 during the shifts. 2 SO_2(g) + O_2(g) 2 SO_3(g) Increase the partial pressure of O_2 (increase the concentration of O_2) Increase the partial pressure of SO_3 (increase the concentration of SO_3). Increase the overall total pressure of the system.Explanation / Answer
A)
increasing P-O2 will favour products, i..e more production of SO3, therefore, SO2 partial pressure will decrease, since it will react to form more SO3
b)
Increaseing the product, will shit to left, then reactants increases
Partial PRessure of SO2 will increase
c)
increasing PRessure in the system will --> favour the least mol production
that is, the right side, then SO2 partial pressure will decrease eventually
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.