I am given the following equation:
Co(Cl)42-(aq) + 6H2O <---> Co(OH2)62+(aq) + 4Cl-(aq)
I know that the solution is blue at elevated temperatures and pink at or below room temperature. I also know that Co(OH2)62+ is pink and that
Co(Cl)42- is blue.
I am asked to predict the color of the reaction mixture at 85 degrees, if the forward reaction is endothermic and to explain why. I think that if it is endothermic then it will be blue, and pink if it is exothermic due to the color of the reactants and products. Also, if it is endothermic, then it is absorbing heat, so the energy will be on the reactants side and vice versa.
Unfortunately this is for a lab class that is weeks ahead of my lecture so I am forced to teach myself these concepts. I get the idea of how concentration, temperature, and catalysts can change the equilibrium in a hypothetical situation. However, I have not seen it applied without dealing with strict values. Anyone care to explain to get me off the ground and running?