in a lab I did a section on \"equilibria in saturated solutions\". in a test tub
ID: 619009 • Letter: I
Question
in a lab I did a section on "equilibria in saturated solutions". in a test tube we mixed 1M of K2CrO4 with 0.1 M BaCl2, the resulting mixture gave us a creamy yellow coloured solution with a precipitate suspended in the solution. Then we added 6 M of HCl drop wise to the solution. I don't think we added enough HCl because nothing really happemed, if we were to add more HCl what would have happened? some people said that the precipitate disappeared and the solution went back to a bright orange/yellow clear colour, what is the chemical equation that describes both these reactions, and how does La Chatelier's principle relate to this?Explanation / Answer
It states that any change made to the system will force the system to partially compensate the change. To increase yield you could: Increase the temperature of an endothermic reaction, because in endothermic reaction, energy is absorbed. Therefore, and increase int temperature increases the product yield. Decrease the temperature for an exothermic reaction, because in this reaction, energy is given off. So to take away the energy, the product forming reaction is favored. For Gas systems, increasing the pressure (in turn, decreasing the volume) will favor the side with the least number of moles. So if the product side has less moles, it will go forward. Likewise, if the products have more moles, decreasing the pressure or increasing the volume of the solution with favor the forward reaction. In aqueous solutions, adding water lowers the concentrations of all the components. To increase the concentration, the system will go to the side with the greatest moles to favor the forward reaction. Adding a catalyst WILL NEVER INCREASE THE Yield. Neither will a inert gas.
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