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Explain how to recognize the conditions under which changes in pressure would affect systems at equilibrium.
In the container, the pressure is caused due to gas molecules which are in continuous motion and hence keep hitting the walls. The pressure experienced will be directly proportional to number of molecules. When the reaction is involving different number of moles of gaseous molecules on the reactant and product side, change in pressure will lead to affect the system at equilibrium. If for a reaction gas molecules of reactant is more than that of product side, then on increasing the pressure equilibrium will shift to the product side where gas molecules are less in number. For the reactions having more number of gas molecules on the reactant side, the increase in pressure will move the equilibrium in forward direction.
Chemistry 102
Chapter 13
Fundamental Equilibrium Concepts
Chemical Equilibrium
Aqueous Equilibria
University of Central Florida
Drexel University
University of Maryland - University College
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everyone, this is Ricky. And today we're gonna be working on a problem 32. And so be be explaining how to recognize conditions under which changes in pressure would effect would affect systems at equilibrium. So pressure, um, is caused by molecules bouncing against the walls of the container and against each other. And so when we have a system that has, for example, maybe two moles of gas on the left and five moles of gas all right, and we increase pressure, we're going to shift equilibrium to the left because of the shot liaise principle, um, saying that a system will try to make a rebound when there's a external force applied. And so in this case, were increasing pressure. So the way that we would decrease pressure is to shift to the left. And so, um, pressure has a difference on equilibrium when we have different numbers of moles of gas and the products of the reactions lips. But he was helpful. See, on the next one
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