![]() This shift in the equilibrium will turn the solution blue, the color of the #CoCl_4^(2-)# ion. the solution is being heated, the equilibrium will shift in the direction of the products. We can say that heat is a reactant in this equilibrium. ![]() The forward reaction is endothermic, which means the equilibrium could be written as The #^(2+)# ion is pink, while the #CoCl_4^(2-)# ion is blue. In aqueous solution, the following equilibrium will be established between the following two ions: When dissolved in water, both #"CoCl"_2#, and #"CoCl"_2*6"H"_2"O"# will produce the complex ion #^(2+)#. The main species involved in the reaction is cobalt (II) chloride, or #"CoCl"_2#, which usually comes in the form of a hexahydrate, #"CoCl"_2*6"H"_2"O"#. Learning Target Log Update Update your LT Log for LT’s 8.7-8.Yes, the color changes that accompany the heating or cooling of the equilibrium mixture are very much in accordance with Le Chatelier's Principle. Therefore, based on the color of the reaction mixture we can conjecture if Keq is greater than or less than 1.” Keq 1 the equilibrium lies to the right, and if Keq ![]()
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