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From the data table determine the rate law for reactions 1-4 and calculate the value of k for each. Thanks
Reactants 8 ml 30% HO, 2 mL 05MK 8 mL 30% H0, 2 mL 0 25 MKO 8 ml 15 HO, 2 mL 0 5 MI 8mL 30% H2O2 2 mL 05MK Temperature Initia

I-IV

BACKGROUND INFORMATION
Given: 3% H2O2 Concentration= 0.88M & 1.5% H2O2 Concentration= 0.44 M


DA VISU Calculate molarity of a 3% mass/volume H₂O2(1,2,4) solution and a 1.5% mass/volume H₂O2 sol. (Part 3) necord these va

•Calculation of H2O2 after mixing for parts I,II, IV= 0.704 M
•Calculation of I^- after mixing for parts I,II, IV= 0.10 M
•Calculation of Initial (mol/L-s)
Torta Covert tomp to K 25° + 273-298 35 +273=308 l M=01903 - 0.1803 13 U1863 (3% H₂O2 = 0.98M ( [H₂O2 ] = 0.88 M * 8ml 50.704
Filled in Table
DATA TABLE Part Reactants 8 mL 3.0% H2O2 + 2 mL 0.5 MKI 8 ml 3.0% H2O2 + 2 mL 0.25MKI 8 ml 1.5% H2O2 + 2 mL 0.5 MKI 8 mL 3.0%
DATA TABLE Part Reactants Temperature (°C) Initial rate (kPa/s) |- 8 mL 3.0% H2O2 + 2 mL 0.5 M KI = 8 mL 3.0% H2O2 + 2 mL 0.2

Now the solutions for Rate Order and Rate Constant are needed


The Decomposition of Hydrogen Peroxide 2. To determine the rate order with respect to H2O2 compare the rates of part I to par
Rate Constant 1. To calculate the value of k, the rate constant, you simply plug into the rate law the values of the concentr
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Answer #1

Solution Melanity of 3.1. H2O2 = 0.88 m Molarity 81574202 = 0.44 m Totul volume of schalim = 10 mL Table : obsevation initial.. ..... . RLON HON D E R WERDE for part (1) males of KI = 2ml x 12 x 0.5 mol ) 1ooom - 1.ox 103 mol. (15) Concentration of HAT ! ... . . ....... ... . . . . Conversion of initial rate from ke fals to mol/l-s PV = nRT :p= ( RT p= CRT, where (= concenorder of Reaction T + 2H202 - H20 + O2(g) . Rate = k [1] 4:08] from Table - 2 Vis * [0.70] [ 0.13 Y, = k [ 344 ( ver] . Se esAgain from Table 1 V = K[ 0.352) [oi] . - r - 10.704)a (2) 2.478x105 Mens = oja 7.27X 105 or 24 = 7,277 = 2.9319 2.478 a (ltale of reaction and Rare constant (k) From Table ① For Part (1) n=k (0.764) 10.1) 7.277X1015 - k X0.05906 k = 7.277x165 = 12

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