CHEM LAB : Iodination of Acetone Question Sheet
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For questions 1 through 3, consider the reaction and experimental data below: ?(?) + ??(??) → ??(?) + ??(?) Experimental Trial [ A ] ( M ) [ B ] ( M ) Initial Rate ( M / s ) 1 1.84 2.37 0.0 ... 341 2 3.27 2.37 0.103 3 1.84 5.47 0.0834 Table 1 - Sample Kinetic Rate Data for the Indicated Reaction Write out the general rate law for the given reaction by using the following symbols: [A] - the concentration of A; [B] - the concentration of B; k - the rate constant; x - the exponent for the [A]; y - the exponent for the [B]. ???? = k[A]x[B]y Divide the rate law for experiment 1 by the rate law for experiment 2 and simplify the resulting expression by cancelling out all constant values. Do NOT insert any numbers. Two items will cancel each other out and you will be left with one set of concentrations and one exponent. ????? = ????? 0.0341/0.103 = (k〖[1.84]〗^x 〖[2.37]〗^y)/(k〖[3.27]〗^x 〖[2.37]〗^y ) 0.0341/0.103 = 〖[1.84]〗^x/〖[3.27]〗^x Algebraically solve the above, simplified expression for x in terms of rate1, rate2, [A]1, and [A]2. Hint: recall the properties of logarithms. Do NOT insert any numbers. 〖rate〗_1/〖rate〗_2 = 〖[1.84]〗^x/〖[3.27]〗^x 0.0341/0.103= 〖[1.84]〗^x/〖[3.27]〗^x [Show More]
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