In second test, the student placed a ing a pink equilibrium mixture in a hot-wat

Question

In second test, the student placed a ing a pink equilibrium mixture in a hot-water bath. The solution turned blue. When the student removed the test tube from the hot-water bath and placed it in an ice-water bath, the solution turned pink. a test tube contain- (2) Is the forward reaction in the [CoClaion/ [Co(H2O)s ion equilibrium exothermic or endother- mic? (3) Briefly explain how the student's observa- tions support your answer to (2). elc rp ag (4) Write the net ionic equation for this equilib- rium, including heat. name

Explanation / Answer

When test tube containing (CoCl4)2-/(Co(H2O)6)2+ equilibrium mixture is placed in hot bath the colour was in pink whereas when it is placed in cold bath the colour changes to blue colour.

This is due to reversible reaction and an endothermic reaction.

ice

(Co(H2O)6)2+(aq) (pink) + 4Cl- ? (CoCl4)2-(aq) (blue) + 6H2O(l)

heat

This is due to the effect of temperature on the reaction. According to Lechatlier principle the equilbrium shifts to either side when disturbance occurs in the reaction. The disturbance here is temperature when there is increase in temperature through heat there is a shift in equilbrium reversibly (exothermic) and and when heat is removed /temperature is lowered the shift in equilbrium to the forward direction (endothermic)

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