Trial 1 5 Data: 2 3 Table 1. Volumes of reactants used for each trial Trial 1 2 3 4 5 KIO3 volume 1.0 mL NaHSO3 volume Table 2. Experimental data for each trial 1.0 mL Show of 1.0 mL orain 2.0ml 1.0ml Loml H₂SO4 volume 1.0 mL 1.0 mL intorant 1.0ml 2.0L 1.0ML 2cr0 1.0MI 1.0ML 2.0m zevo 1.0 mL H₂O volume [H₂SO4]0 1.0 mL Room Temperature = 19.0°C In [K103] stock = 0.020 M (ml) [K103] = 2010 1.0 mL Starch volume 1.0 mL 91 PRITET DHE 200 1.0 mL [NaHSO3]Stock = 0.030M (mi) [Notiso₂] = final AUT [H₂50₁] = 0.020m "(ml [H₂SQ₂4]final (ml) H₂0 1.0 mL 1.0 mL 1.0 mL Ice-bath temperature = Time (s) (Run 2) Total Volume 5.0 mL 7100 Time (s) [KIO3]0 [NaHSO3]0 (Run 1) 4.01.10 -3M 4.0x1040x10 ³28.015 38.385 30.115 32.175 & QXID-M4.0XID M 4.0x10 3 11.5SS 10.885 10.935 11.12s 4.OKIDM 8.0x10M4.0X10 19.505 21.215 24.33321.685 4.0x10 4.0x108.0 X10 M 21.15s 22.00$ 12.835 20.665 4.0X10 4.0x 104.0x1031.27.9 1:06.75 1:31.80 82.165 M 5.0 mL 5.0 mL 5.0 mL 5.0 mL Time (s) (Run 3) Average Time (s) -1.0°C Calculations: 1. Show the dilution calcu [KI03 ]= 0.000 [KIÖ3]= + Imi starch - Total y = 5.00 ml 0.0 [termine the 10.03 [NaHSO3]=0.0. the reaction ra 5- 100 KI0g added (ast Ime Nukso Ime H₂SO4 IML H₂O Fimi Starch 2. 4.god show work Formula ₁V₁= M₂ Vz [KI0₂]==0.000m (0.020) (0.001) = (0.005)=0.004 moll (ml) = (0.30)(0.005) = (0.0051) = 0.000 mol/L (ml) = (0.30)(0.001) = (0.005)=0.00u mol/L [tb₂s0y + -10:0201 (0.001) = (0.005) = 0.04 mol [NaHsQ3]=0.000M 2. Determine the reaction rates for the following trials. Your answers should contain correct units. You must show work to receive full credit. Rate= (-1/10) X (0-0.004) 132.175=1.24 x 10 m/s Calculations: 1. Show the dilution calculation for Trial 2.) [KI03 ] = 0.020 M (mi) = Trial 2: Trial 3: Trial 4: Trial 5: Rate = (-1/10) x (0-0.004)/11.12=3.59x-5 m/s Rate = Rate (-1/10) x (0-0-004)/21.68 = 1.84x-5 m/s (-1/10) x (0-0.004)120.66=1.93-5 m/s -6 Rate = - (-1/10) x (0-0.004) | 82.16 = 4.86** 3 m/s Ju J to receive full credit. 4. Determination of the Rate Constant at Room Temperature Use the rate law you determined in step 3 to calculate the rate constant (with units) for Trial 1. Report answers in Table 3. Show your work for Trial 1 to receive full credit. Repeat this calculation for trials 2-4 and report answers in Table 3. rate = k [K10₂] (NaHSO3 ] [H₂SO4] 1.24x10-5 = x (0.0040) (0.0040) (0.0040) Table 3: Determined rate constant at room temperature for Trials 1 - 4. 1.24x10-5 Rate constant (k) Trial 1 2 4 Average: elsiu Rate = les brawl sé snutmat moon orb galet sonoo ad adw an dans to moite 2 lanT bns I Isi ni eqmst instal nozeo odi nicigx Sinetenos odt bib worl Write the overall rate law for the reaction using your average rate constant (calculated in Table 3). Report answer with proper units. be sier notion or pets 5. Determination of the Rate Constant at the Lower Temperature Tnal 5 sau 2 b Rupo 2uino IN lainT ni samo ist bevisado y no bons Use the rate law you determined in step 3 to calculate the rate constant (with proper units) for the trial conducted at the lower temperature. Show your work to receive full credit. 5 6 L F X 1 8 Y 8 option 14 G C ( 6 n 0 - H O d K 1 > Determine "c": . Determine "b": 4.0X10-3 8.0v 10-3 A. Determine "a" Thall Tral 2 1.54 x 10-5 3.59x10-5 ? rate= K [ko] [NaHSO3] [H₂SO4 ] 3. Determine the orders using the rate law for the reaction. You must show work in order to receive full credit. ✓ mand # option vale T1 = [K]0₂39 [NaHSO3]b[H₂SO4) C rate Ta X (KIOJ[NaHSO3] [H₂SO4) (4.0x10-3]ª[4.0X10-3 340103] -S 23.59x107 0-5 31.84X107 41.93 x 10-5 5 4.86 x 10-6 Trial [8.0X10-3][4.0×10-³][4.00 1031 1.24x10-5