Question

I. Write the equilibrium constant expression, K for the following reaction Fe"(ag) FENCS(ag) SCN (ag) + CFENCS D 2. In part A of Experiment 34, it was assumed that all of the SCN added to the reaction mixture was converted to product (FeNCS). Which of the following best explains why that assumption was valid? A) The moles of Fe added equaled the moles of SCN- added. B) In part A, the SCN was the limiting reactant whereas in part B, it was not. C) There was a large excess of Fe * in Part A, ensuring that alll of the SCN-was consumed. D) In part A, the concentrations of SCN were much higher ensuring that the reaction was complete. S 3. In part B of the experiment, how were the concentrations of FeNCSa determined? A) They were determined using the moles formed and the total volume of the solution. B)They were detemined using the measured absorbance values and the calibration curve from Part A C) They were determined by subtracting thee reacted moles from the initial moles for both reactants. D) They were determined using the dilution formula and the volumes used in the experiment. 4, Name the following compounds. a) Fe(NO;) Tron m) NHrate ) NeSCN S0dion th peyanate ) HNO:(am acid) it acid 5. A 1.0 mL aliquot of 0.0020 M NaSCN was diluted to 50.0 mL with 0.1 M HNO3. Calculate the moles of SCN-added and the molar concentration of SCN- in the diluted solution.

Answer 1

Malaruty a SCN ions = 0.0020M Initial valume I ml M ales Vellin itus) Melauity Meles 1x10-3 I10-3 1 1o3 Males 210-0 Se malus h SCN addid aue 2xIomous. final valume of aftur dilutian =50ml Maus 2 xIO6 mix Malar cancn taatian(mal oity) scN in diuted salution 2x10-4 1 50x10-3 ox105 4x10-5 Wh0000.0