Introduction: In this lab, seven test tubes containing solutions in equilibrium had different stresses added to them to examine the balance in each example. The purpose of the experiment was to indentify the details of shifting in equilibrium reactions and determine how the adding of a stress can affect a reaction. A chemical reaction that is in equilibrium is reversible, where a reactants can create products and products can go back to products. Equilibrium is reached when the rate of a forward reaction is the same as the reverse reaction and the concentration of the reactants and products are equal. In a written reaction, equilibrium is represented by two arrows going in opposite directions between the products and the reactants. Adding or reducing either heat, pressure, a reactant, or a product can distrub the balance of a reaction in equilibrium. Le
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Cl- has the common ion sources of HCl and CaCl2 in test tubes C and D.
Le Chatelier’s Principle explains that adding Cl- as a reactant will shift the equilibrium to the right to produce more product from the added reactant in test tubes C and D.
When adding acetone to test tube E, it changed the solution from pink to blue because CoCl42- was formed on the product side, producing a right shift. Le Chatelier’s Principle states that the removing of water, because of the acetone, will cause the addition of more product to make up for it.
When heat was added to test tube B, the solution changed from pink to blue because CoCl42- was made, a right shift. Removing the heat or cooling the solution in test tube C made it go from blue to purple because of the forming of Co(H2O)62+ comple ions, a left shift.
Adding heat to test tube B caused the solution to go from pink to blue, a right shift, meaning heat would have to be a reactant.
Adding the heat caused the reaction to be
Cl- has the common ion sources of HCl and CaCl2 in test tubes C and D.
Le Chatelier’s Principle explains that adding Cl- as a reactant will shift the equilibrium to the right to produce more product from the added reactant in test tubes C and D.
When adding acetone to test tube E, it changed the solution from pink to blue because CoCl42- was formed on the product side, producing a right shift. Le Chatelier’s Principle states that the removing of water, because of the acetone, will cause the addition of more product to make up for it.
When heat was added to test tube B, the solution changed from pink to blue because CoCl42- was made, a right shift. Removing the heat or cooling the solution in test tube C made it go from blue to purple because of the forming of Co(H2O)62+ comple ions, a left shift.
Adding heat to test tube B caused the solution to go from pink to blue, a right shift, meaning heat would have to be a reactant.
Adding the heat caused the reaction to be