In this lab, I have to answer questions using pictures of colors of different reactions and Le Chatlier's principle.
Here are the lab questions with my responses italicized.
A. Put 50 mL of 0.0005 M KSCN solution in a beaker and observe the appearance. Add 5 drops of 0.2 M Fe(NO3)2 solution and observe the appearance. What evidence is there for a chemical reaction? KSCN originally appears clear and Fe(NO3)2 originally exhibits an orange color. The product (the right beaker in the right slide) has a different color, a shade of red, than either of the two reactants.
The observed reaction is Fe2+ (aq) + SCN- (aq) → FeSCN+ (aq)
Identify the color of each reactant and product.Fe2+ (aq) is orange, SCN- is transparent and has no color, and FeSCN+ is red.
B. Fill three large test tubes 1/3 full with the solution from part IA. Keep one test tube unchanged to use as a standard for comparison. To the second test tube, add a few crystals of solid KSCN (source of SCN-) . Add one drop of Fe(NO3)2 (source of Fe2+) to the third test tube. Record your observations.The first test tube that maintains the same solution in 1A keeps its red-orange color. The second test tube with the crystals of KSCN exhibits a very dark, red color. The third test tube with the drop of Fe(NO3)2 has a more prominent and slightly darker shade of red than the first test tube.
C. Consider the reaction Fe2+ (aq) + SCN- (aq) → FeSCN+ (aq)
Is this reaction 100 % complete with one limiting reactant, or is it fractionally complete (at equilibrium) with neither reactant limiting? Explain your reasoning in detail.No answer right now
I am stuck on answering part C. Do the different colors in test tubes 2 and 3 indicate that the reaction is NOT complete? Before answering, could you also verify my repsonses for questions A and B?