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# Kinetics informal - Kinetics Theory Lab Olivia Downs CHM 1046L/85606 The purpose of this experiment was to determine rates of iodide ions with

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Kinetics Theory Lab Olivia Downs 3/21/11 CHM 1046L/85606 The purpose of this experiment was to determine rates of iodide ions with peroxodisulfate ions to calculate orders to find the rate constant “k”. Also, we found the activation energy, frequency factor, and measured the effect of a catalyst on the rate of reaction. Data of the effect of a catalyst (Cu(NO3)2) on the reaction Trial Temp ˚C Time(sec) Avg. Time(sec) 13 25˚C 21.2, 24.1, 24.3 23.2 14 25˚C 47.3, 40.6, 44.6 44.2 15 23˚C 63.0, 58.9, 56.9 59.6 16 23˚C 127.0, 114.0, 112.0 117.7 Data of Part III Trial KI (NH4)2S2O8 Rate avg Rate constant (k) Ratio of k values 13 .084 .042 2.72E-5 7.710E-3 k13/k1=0.49 14 .042 .042 1.43E-5 8.102E-3 k14/k2=1.41 15 .042 .042 1.06E-5 1.202E-2 k15/k3=2.90 16 .042 .042 5.37E-6 1.162E-2 k16/k4=3.47 Calculating concentrations of [I-], [S2O8^2-], [S2O3^2-] M1V1=M2V2 Dilution formula (.008L)× (.2M) ÷ (.019L) = .084210526 = .084 I^- (.004L)× (.2M) ÷ (.019L) = .042105263

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= .042 S2O8^2- = .084 S2O3^2- Calculating the rate with respect to [S2O3^2-] ½ × .084 ÷ 93 =5.54E-5 s^1 Calculating the order with respect to [I-] = 2.455530683 =2.4514 Calculating the order with respect to [S2O8^2-] = 1.148863386 =1.1473 Calculating the rate constant for Trial 1 Rate constant= k ÷ [.084]^1.721[.042]^1.250 (5.54e-5) ÷ [.084]^1.721[.042]^1.250 K= 1.571e-2 s^-1 Complete rate law Rate law= 5.953e-3[I^-]^1.721[S2O8]^1.250 Calculating Activation energy Slope= -E(a)/R Slope × R= -Ea (8.314)(-3060.1)= -25442 E(a)= 25442 kJ/mol Calculating Frequency factor A= k/e^-E(a)/RT (5.54e-5) ÷ e^(-25442 ÷ (8.314)(23))
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## This note was uploaded on 11/03/2011 for the course CHM 1046L taught by Professor Simmons during the Spring '11 term at Tallahassee Community College.

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Kinetics informal - Kinetics Theory Lab Olivia Downs CHM 1046L/85606 The purpose of this experiment was to determine rates of iodide ions with

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