The next photo will show what was initially added to all the tubes and then what

Question

The next photo will show what was initially added to all the tubes and then what was added individually to each tube

Tube 1 resulted in a stronger color change which means a shift toward products

Tube 2 results in a weaker color change so a shift towards reactants

Tube 3 resulted in a stronger color change so shift towards products

Tube 4 resulted in a weaker color change so shift towards reactants

Questions 1. For Part 1, you determined whether each action you performed caused the reaction's equilibrium to shift toward the products or the reactants, if at all. Explain your observations in Tubes 1-4, based on Le Chatelier's Principle.

Explanation / Answer

The tubes originally have Fe(NO3)3 + KSCN

1. The first one shift to the right because you increse the concentration of FeNO3, doing this increases the effective collisions of the reactants and this will increase the concentration of products.

2. In the reaction you will produce some KNO3, soo if you add KNO3 to the solution this will increase the concentration of the reactants (left)

3. This is similar to point 1, you will increase the effective collisions of reactant to get more product. (right)

4. Some of the Hg+2 will react with the SCN- so you will decrease the number of collisions to produce FeSCN+2 this is why you get a weaker color, the reaction shifts to the left.

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