First let me point out that isocyanate is NOT SCN. I realize those are parts of the same question and you may have been asking two questions. I so you will need to clarify for me.
A + B ==> C + heat.
If the temperature is raised the reaction will shift to the left.
If the reaction is
Fe^+3 + SCN^- ==> FeSCN^+2 and the reaction shifts to the left, I would expect the intensity of the color to be less since less of the complex is present at the higher temperature.
The reaction of the ferric ions with isocyanate ions is an exothermic reaction. In what direction would you expect the equilibrium to move if the solution temperature is raised? Would the color of the reaction intensify? Explain.
What would happen if you decreased the concentration of SCN-(aq). In which directions would the equilibrium move?
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It is part of the same question just two different parts.
OK. My response above stands but isocyanate and SCN are not the same thing.
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