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: 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.

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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.


Tube

Photos

Observations

1

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  • Tube 1 is the control in the experiment.
  • The color is a between red and orange, this is the product from the first reaction.
  • At this point the equation is at equilibrium.
  • [FeCl3] constant
  • [KSCN] constant
  • [Fe(SCN)6]K3constant
  • [KCl] constant

2

image04.jpg

  • Tube 2 has 20 drops of 0.1 M FeCl3.
  • Additional iron (III) chloride (FeCl3) was added to the system. The stress is too much FeCl3. The equilibrium will shift to the right, towards products, in order to remove the excess FeCl3.
  • [FeCl3] increases
  • [KSCN] decreases
  • [Fe(SCN)6]K3increases
  • [KCl] increases

3

image04.jpg

  • Tube 3 have 20 drops of 0.1 M KSCN
  • When we increase the concentration of KSCN, the system will shift to the right in order to produce less of KSCN and continue with equilibrium.
  •  [KSCN] increases
  • [FeCl3] decreases
  • [Fe(SCN)6]K3increases
  • [KCl] increases

4

image04.jpg

  • And tube 4 have 1 g of KCl crystals.
  • When we added KCL (product) then the reaction shift to the left as a reestablish to the equilibrium, by consuming part of the added substance.
  • [KCl] increases
  • [KSCN] increases
  • [FeCl3] increases
  • [Fe(SCN)6]K3decreases


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