Why is Le Chatelier's principle important?
Le Chatelier's Principle is important, because it allows us to shift an equilibrium to the side that we would like to favor. For example the Haber Process produces ammonia reversibly.
The reaction is run at high pressures, because there are 2 moles of ammonia on the product side, but 4 moles of gas on the reactant side (3 mol of hydrogen and 1 mol of nitrogen). Since 2 mol of gas occupies a smaller volume than 4, increasing the pressure will increase the amount of ammonia at equilibrium. Interestingly, high temperatures favors the reactant side, but the reaction will reach equilibrium faster at higher temperatures, which is why the reaction is carried out at a moderately high temperature. For more, see: What is Le Chatelier's principle?
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Le Chatelier's principle is important because it helps predict how a system at equilibrium will respond to changes in temperature, pressure, or concentration. This understanding allows for the manipulation and optimization of chemical reactions and processes in various fields such as industrial chemistry, environmental science, and pharmaceuticals.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
- Excess PbBr2(s) is placed in water at 25 C. At equilibrium, the solution contains 0.012 M Pb 2+(aq). What is the equilibrium constant for the following reaction? PbBr2(s) --> Pb2+(aq) + 2Br-(aq)
- What volume of water is required to dissolve a #6.7*g# mass of #"calcium sulfate"# if #K_(sp)*CaSO_4=2.4xx10^-5#?
- How do we use #K_"sp"# values for solubility calculations....?
- How does the equilibrium evolve if the pressure of reactants or products are altered?
- How is Le Chatelier's principle used to treat CO poisoning?

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