potassium chromate to dichromate I am trying to detemine if the reaction in the

Question

potassium chromate to dichromate

I am trying to detemine if the reaction in the photo is endothermic or exothermic.

I’ve performed the experiment of adding HCl to the initial potassium chromate to observe the colour change from yellow to orange, as more H+ were present and therefore used to shift the equillibrium to the right.

I’ve also performed the experiment of submerging the solution in an ice bath and a heat bath for the purpose of observing colour change (reactants favoured=yellow; products favoured=orange). However, even though I’ve done this three times, no colour change was observed??

There was a precipitate when submerged in the ice bath, which my best guess is KCl salt.

This would mean that upon removal of heat, more products were created. So an exothermic reaction??

What’s the best way for me to quantify this so I can be sure? Help! (And thanks)

Molecular Equation: Potassium Chromate Dichromate (at equilibrium) + OH-(from NaOH) H2O (product) 1 Net Ionic Equation: 2Cr04 2-(aq) + 2H+ (aq)--Cr207 2-(aq) + H20(1)

Explanation / Answer

I believe that the reaction is endothermic, the cold seprared them, returning the color to its original state, while the heat returned it to the product color.

Also the substance became more acidic which equals to higher heat energy.

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