Kinetics of Crystal VioletCatherine Lozier04/02/2013Chem 1310 Section C02TA Ryan BucherLab Partners:Chelsey Arnold Sunya MorinTran GHonor Pledge: I did not copy this work from any others student(s), current students in lab or old lab reports ________________________________________________SignatureDATA AND OBSERVATIONSKinetic Runs at Room TemperatureActual Temperature (°C)Run 1 20.0 Run 2 20.0Kinetic Runs at Room TemperatureTime (s) Run 1 Run 20 0.856 0.90120 0.794 0.87640 0.743 0.84660 0.702 0.82280 0.654 0.796100 0.613 0.771120 0.574 0.746140 0.538 0.723160 0.506 0.699180 0.475 0.676200 0.444 0.654220 0.417 0.636240 0.391 0.612260 0.368 0.592280 0.345 0.571300 0.322 0.551320 0.303 0.533340 0.284 0.514360 0.266 0.497380 0.249 0.478400 0.234 0.460420 0.219 0.444440 0.206 0.429460 0.194 0.416480 0.182 0.404500 0.170 0.390520 0.160 0.380540 0.150 0.368560 0.141 0.356580 0.131 0.345600 0.124 0.335Kinetic Runs at Room TemperatureTime (s) Run 1 Ln(Run 1) 1/Run 10 0.856 -0.155 1.16820 0.794 -0.231 1.25940 0.743 -0.297 1.34660 0.702 -0.354 1.42580 0.654 -0.425 1.529100 0.613 -0.489 1.631120 0.574 -0.555 1.742140 0.538 -0.620 1.859160 0.506 -0.681 1.976180 0.475 -0.744 2.105200 0.444 -0.812 2.252220 0.417 -0.875 2.398240 0.391 -0.939 2.558260 0.368 -1.000 2.717280 0.345 -1.064 2.899300 0.322 -1.133 3.106320 0.303 -1.194 3.300340 0.284 -1.259 3.521360 0.266 -1.324 3.759380 0.249 -1.390 4.016400 0.234 -1.452 4.274420 0.219 -1.519 4.566440 0.206 -1.580 4.854460 0.194 -1.640 5.155480 0.182 -1.704 5.495500 0.17 -1.772 5.882520 0.16 -1.833 6.250540 0.15 -1.897 6.667560 0.141 -1.959 7.092580 0.131 -2.033 7.634600 0.124 -2.087 8.0650 100 200 300 400 500 600 70000.10.20.30.40.50.60.70.80.9f(x) = − 0x + 0.72R² = 0.94Absorbance v. TimeTime (s)Absorbance Readings0 100 200 300 400 500 600 700-2.5-2-1.5-1-0.50f(x) = − 0x − 0.17R² = 1Natural Log of Absorbance v. TimeTime (s)ln (Absorbance Readings)0 100 200 300 400 500 600 7000123456789f(x) = 0.01x + 0.35R² = 0.941/Absorbance v. TimeTime (s)1/ (Absorbance Readings)Temp (K) kobs1/Temp(K) ln(kobs)Run 1 293 0.00320.003413 -5.7446045Run 3 305 0.00480.0032787 -5.3391394Run 4 315 0.00570.0031746 -5.1672891Run 5 325 0.00860.0030769 -4.7559931Time (s) Run 1 Run 2 Run 3 Run 4 Run 50 0.856 0.901 0.495 0.615 0.44910 - - 0.469 0.572 0.40120 0.794 0.876 0.448 0.536 0.35930 - - 0.427 0.505 0.32640 0.743 0.846 0.404 0.474 0.29650 - - 0.383 0.446 0.26760 0.702 0.822 0.366 0.422 0.24370 - - 0.347 0.397 0.22080 0.654 0.796 0.331 0.374 0.20190 - - 0.314 0.354 0.185100 0.613 0.771 0.299 0.335 0.169110 - - 0.285 0.316 0.156120 0.574 0.746 0.272 0.300 0.142130 - - 0.259 0.284 0.132140 0.538 0.723 0.247 0.269 0.122150 - - 0.236 0.251 0.113160 0.506 0.699 0.226 0.239 0.106170 - - 0.215 0.226 0.099180 0.475 0.676 0.206 0.214 0.092190 - - 0.197 0.203 0.087200 0.444 0.654 0.189 0.196 0.080220 0.417 0.636 - - -240 0.391 0.612 - - -260 0.368 0.592 - - -280 0.345 0.571 - - -300 0.322 0.551 - - -320 0.303 0.533 - - -340 0.284 0.514 - - -360 0.266 0.497 - - -380 0.249 0.478 - - -400 0.234 0.460 - - -420 0.219 0.444 - - -440 0.206 0.429 - - -460 0.194 0.416 - - -480 0.182 0.404 - - -500 0.170 0.390 - - -520 0.160 0.380 - - -540 0.150 0.368 - - -560 0.141 0.356 - - -580 0.131 0.345 - - -600 0.124 0.335 - - -Kinetic Runs at Higher TemperatureActual Temperature (°C)Run 3 35 Run 4 45 Run 5 550 0 0 0 0 0 0 0 0-5.9-5.7-5.5-5.3-5.1-4.9-4.7-4.5f(x) = − 2812.81x + 3.85R² = 0.98ln(kobs) vs. 1/Temp (K-1)1/Temperature (K-1)ln(kobs)SAMPLE CALCULATIONS1. Kobs = k[OH-]n0.0032/0.0017 = kint[0.1]n/kint[0.05]n1.8824 = 2nN = 0.9126  12. Kobs = kint[OH-]n0.0032 = kint[0.1]1Kint = 0.0323. Ln(k) = -Ea/R * 1/T + ln(A)Y = -Ea/R * x + ln(A)Y = -2812.8x + 3.8499-Ea/R = -2812.8Ea = 2812.8 * 8.314*10-3 kJ/molKEa = 23.39 J4. Ln(k) = -Ea/R * 1/T + ln(A)Y = -Ea/R * x + ln(A)Y = -2812.8x + 3.8499Ln(A) = 3.8499A = 46.995. T1/2 = 0.693/kobsT1/2 = 0.693/0.0032T1/2 = 216.5 sDISCUSSIONThe objective of lab 11 was to experimentally determine the kinetic rate for the reaction between crystal violet and sodium hydroxide at room temperature, as well as calculate the activation energy and half-life of the reaction. Because the graph of the natural log of absorbance was the most linear, the m value was determined to be 1. The R2 value of the linear regression of the natural log graph was 1, which indicates an exact linear relationship between the variables, and that there was little to no random error in the data. Based on the linear regression line, then-value was calculated to be 0.9162. For further calculations, this was rounded up to 1, which may have influenced the accuracy of the kint calculations. Kint was calculated to be 0.032. The activation energy of the reaction was calculated to be 23.39 J, and A is 46.99. The first run of the reaction has an experimental half-life of 216.5 s, which is consistent with the data. Any systematic error in the measurements would be attributed to improper calibration of the spectrometer.REFERENCES Lab ManualChemistry for Engineering Students, Second Edition. Lawrence S. Brown, Thomas A.