• anonymous
6. In real life, a given system can approach equilibrium from different starting points but will still have the same equilibrium constant. How is this possible? Explain your answer in complete sentences.
  • Stacey Warren - Expert
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  • schrodinger
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  • anonymous
At a given temperature a given reaction will have a k value (equilibrium constant), and this will stay constant. What this means is that the amount of product you will make will change because the k value cannot. For example you have a reaction that has reached equilibrium, but you decide to add more of whatever you're products were, you're equilibrium will shift to make more reactant. This is what is known as La Shatliere's principle (there is no way that's spelled right). The reasoning behind this involves a lot of thermodynamics and kinetics knowledge, but this is a start. Hope that was helpful, i think that awnsers the question u asked, i can specify in certain areas if you want.

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