Observation Sheet: Effect of Concentration on Rate of Reaction Approximate Molarity of stock crystal violet (CV+) solution: 3.00 x 10-5 mol/L 588.5 nm Wavelength of maximum absorbance (Imax): Molar Absorptivity of CV+ at Imax (from advance study assignment): 8.32 x 104 L/mol-cm) 3.00 10-1 mol/L Molarity of NaOH used in Run 1: 2.00 x 10-1 mol/L Molarity of NaOH used in Run 2: Molarity of NaOH used in Run 3: 1.00 x 10-1 mol/L Run 2 Run 1 Time (s) Absorbance Run 3 Time (s) Absorbance Time (s) Absorbance 0 0.898 0 1.048 0 1.138 10 0.736 10 0.920 10 1.064 20 0.604 20 0.807 20 0.994 30 0.495 30 0.708 30 0.930 40 0.406 40 0.622 40 0.869 50 0.333 50 0.545 50 0.813 60 0.273 60 0.479 60 0.760 70 0.223 70 0.420 70 0.711 80 0.183 80 0.369 80 0.664 90 0.150 90 0.323 90 0.621 100 0.123 100 0.284 100 0.581 110 0.101 110 0.249 110 0.543 120 Initial Temp 0.083 Final Temp (C) 23.9 120 Initial Temp (C) 23.7 0.219 Final Temp (C) 24.4 120 Initial Temp (C) 23.8 0.508 Final Temp (C) 24.3 (C) 23.4 8. Explain why the reaction temperature was measured for each run in Experiment M. (0.5) 9. Using the values from Run 1 of Experiment M, determine the value for [OH-] at t=120 s. What percentage of the initial amount of hydroxide is consumed during the 120 seconds? Is this consistent with our treatment of the run as pseudo-first order? (Hint. What amount of [CV] is consumed during this time?) (1.5) 10. If you performed another run in which [OH-]; was identical to [CV+]i, would a plot of In[CV+] versus time reveal a straight-line relationship? Would any of the three types of integrated rate- law plot reveal a linear relationship? Explain your answers. (1.0)