Studying the concentration and temperature effect on anequilibrium: Co(H2O)62+(a
ID: 679277 • Letter: S
Question
Studying the concentration and temperature effect on anequilibrium:Co(H2O)62+(aq) + 4 Cl-(aq) +heat CoCl42-(aq) + 6H2O(l) (Pink ) (Blue ) The color of Co(H2O)62+ insolution is dark purple The color of Co(H2O)62+solution after heating is light purple The color of Co(Cl)4-2 in solution isPurple/black The color of Co(Cl)4-2 solution afterwater is added is pink/purple a) based on the observations on heating this mixture, is thisreaction is exothermic or endothermic? Explain your answer b) What happened to the equilibrium when you added water?Explain your answer keeping in mind that this is an aqueous solution. Studying the concentration and temperature effect on anequilibrium:
Co(H2O)62+(aq) + 4 Cl-(aq) +heat CoCl42-(aq) + 6H2O(l) (Pink ) (Blue ) The color of Co(H2O)62+ insolution is dark purple The color of Co(H2O)62+solution after heating is light purple The color of Co(Cl)4-2 in solution isPurple/black The color of Co(Cl)4-2 solution afterwater is added is pink/purple a) based on the observations on heating this mixture, is thisreaction is exothermic or endothermic? Explain your answer b) What happened to the equilibrium when you added water?Explain your answer keeping in mind that this is an aqueous solution. a) based on the observations on heating this mixture, is thisreaction is exothermic or endothermic? Explain your answer b) What happened to the equilibrium when you added water?Explain your answer keeping in mind that this is an aqueous solution.
Explanation / Answer
a) As heating is required for the forward reaction to proceed, thereaction is endothermic. b) Noe that the water added is in LIQUID state, so that theequilibrium position will not change. Only aqueous solution ofwater is able to make a change in the equilibrium position. Hope this helps!