The equilibrium would heavily skewed the left reactant side

Hypothesis: ​Adding reactants will shift the equilibrium to the right, and

taking away reactants will shift the equilibrium to the left.

Dependent variable: Change of color

Steps:

to the same solution and record the results again.

4. Add CaCl2 to the solution from step 2. Record the results.

Calculations and Analysis:

● in terms of reaction completion- ​the reaction has been

completed at this point

H20 was added and the liquid turned pink.

● explain how the rate change affects the concentrations of the reactants and products at the new equilibrium position- ​the concentration of the reactants increased and the concentration of the products decreased
3. What stress did the addition of AgNO​3 ​cause to the equilibrium system, and how? Explain the resulting shift in equilibrium and changes in concentrations using your observations and data from the experiment.

The equilibrium switched from having more CoCl than Co(H20) to having more Co(H20) than CoCl.

make more reactants or more products? Which of your trials models this? ​More products, trial 3

● If a product was added, did the new equilibrium system shift to make more reactants or more products? Which of your trials models this? ​More reactants, trial 2

When adding heat, the equilibrium would be heavily skewed to the left (reactant) side. When taking away heat, the system would be closer to equilibrium.