: Effect of heat hydrated copper (II) sulphate and subsequent addition of water to the anhydrous product.
Free essay example:
Gabriela Soto
Investigation #9
- Observations for PART A: Effect of heat hydrated copper (II) sulphate and subsequent addition of water to the anhydrous product.
CuSO4 + 5H2O ←→ CuSO4 + 5H2O
At first the color of hydrated copper (II) sulphate was blue when it was hydrated but after we burn it, the color turn into white because the water was evaporated when we heat it. At this moment the equilibrium shit to the left because the increase in temperature (from 20°C to 39°C) pushes the system away from equilibrium and in order to restore equilibrium is need to remove some of this additional heat. Le Châtelier's Principle states that the system will react to remove the added heat, thus the reaction must proceed in the reverse direction: This is an endothermic reaction.
Then we added water to the test tube that contains hydrated copper (II) sulphate and it turned blue again. The equilibrium shift to the right because the temperature was decrease. Because the reaction is exothermic, the reaction produces heat when it proceeds in the forward direction. The forward reaction would thus occur to release heat in a try to balance the heat that was removed from the system.
- Observations PART B: Common ions effect on a chemical equilibrium.
FeCl3 + 6KSCN ←→ [Fe(SCN)6]K3 + 3KCl
FeCl3 and KSCN are colorless, so when we add 1ml of FeCl3 and 1 ml of KSCN into water what we can observe is that the color increase in red coloration.
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