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Equilibrium and Le Chatelier's Principle REPORT SHEET Blank=0.047 Kc Solution Avg Kc (Sol 1-5) 1 1 2 A447 [FENCS?) (M) 360 0.01006817 490 0.000.091/51 533 0.00009923 ,739 0.00013621 1.010 0.0018487 3 4 5 L6 414 0.00007786 2237 0.004009 L7 ICE tables (enter molar concentrations in scientific notation) Sol 1: Fe}"(aq) + SCN'(aq) - FeNCS"(aq) Sol 2: Fe(aq) + SCN"(aq) FeNCS2(aq) 1 1 E E Sol 3: Fe(aq) + SCN (aq) - FeNCS"faq) Sol 4: Fe(aq) + SCN (aq) - FeNCS?" (aa) ! 1 C E E Sol L6: Fe(aq) + SCN'(aq) - FeNCS"(aq) Sol L7: Fe%"(aq) + SCN (aq) FENCS2(aq) 1 ! E E Sol 5: Fe(aq) + SCN (aq) FeNCS2(aq) 1 C E Answer the following by hand on this report sheet. Use complete sentences for Q3, 4 and 5. 1. Solution 4 was at equilibrium then it was disturbed by addition of 0.10 M HNO3 to create solution L7. Show your calculation for the initial reactant concentrations of Fe+ and SCN in solution L7. 2. Calculate Q, the reaction quotient, for L7 immediately after addition of 0.10 M HNO3. Show your work. 3. Compare Q for solution L7 to your average value for Ke for Solutions 1-5. In which direction did the equilibrium shift when equilibrium was reestablished? 4. Compare the equilibrium concentrations of [FeNCS2] for solutions L7 and L6. Offer an explanation for the differences you observe. 5. Compare K, for 16 to the average K, for solutions 1-5. What result do you expect? Offer a justification for your view