Given the following: Solutions 0.04 M KI 1% starch 0.03 M Na2S2O3 0.05 M H₂SO4 0.08 M NaCl and Solutions 0.04 M H2O2 deioinized water Flask 1 25.0 mL 5.00mL 5.50 mL 5.00 mL O O Rate=k[I][H₂O₂] Beaker 1 25.0 mL 0 Calculate the following for each run: • the initial molarities of I and H₂O2 (from the solutions tables) • the rates of reaction [12]/time (calculate the [1₂] from [S₂O32-] and the reaction: 12(aq) + 2 S₂03² (aq) → 21 (aq) +S406² (aq) Choose the correct rate law for this reaction from your calculations. O Rate=k{1]2[H₂O₂] Rate=k[I][H₂O₂]² O Rate=k[1]²[H₂O₂]² Flask 2 25.0 mL 5.00mL 5.50 mL 5.00mL 0 Beaker 2 12.5 mL 12.5 mL Following the procedure Run 1 is when Beaker 1 is added to Flask 1 and the timer is started giving the time recorded for the run in the table below. This is repeated with Beaker 2 and Flask 2 for Run 2 and finally Beaker 3 and Flask 3 for Run 3: The results for these runs are given below: Run Time (seconds) 1 35 2 66 3 72 Flask 3 12.5 mL 5.00mL 5.50 mL 5.00mL 10.0 mL Beaker 3 25.0 mL 0

Given the following: Solutions 0.04 M KI 1% starch 0.03 M Na2S2O3 0.05 M H₂SO4 0.08 M NaCl and Solutions 0.04 M H2O2 deioinized water Flask 1 25.0 mL 5.00mL 5.50 mL 5.00 mL O O Rate=k[I][H₂O₂] Beaker 1 25.0 mL 0 Calculate the following for each run: • the initial molarities of I and H₂O2 (from the solutions tables) • the rates of reaction [12]/time (calculate the [1₂] from [S₂O32-] and the reaction: 12(aq) + 2 S₂03² (aq) → 21 (aq) +S406² (aq) Choose the correct rate law for this reaction from your calculations. O Rate=k{1]2[H₂O₂] Rate=k[I][H₂O₂]² O Rate=k[1]²[H₂O₂]² Flask 2 25.0 mL 5.00mL 5.50 mL 5.00mL 0 Beaker 2 12.5 mL 12.5 mL Following the procedure Run 1 is when Beaker 1 is added to Flask 1 and the timer is started giving the time recorded for the run in the table below. This is repeated with Beaker 2 and Flask 2 for Run 2 and finally Beaker 3 and Flask 3 for Run 3: The results for these runs are given below: Run Time (seconds) 1 35 2 66 3 72 Flask 3 12.5 mL 5.00mL 5.50 mL 5.00mL 10.0 mL Beaker 3 25.0 mL 0

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Saturday March 12, 2022 Inha 3. Find the 9₁ · equilibrium constant, tw, at 25°6 and 40°C. for the following Resution. - OH H₂2₂0=4+ DH (Wallande) Species OGA (kcal/mol) H+ 0 O OH- -54957 -32.595 1₂0 -68.3/79 -56.690 36. Is the Reaction exothermic of endothermic?
4. The Ksp for MgCO3 = 1.1 x 101º. CIRCLE the solubility of MgCO3 in pure water. a) 1.1 x 10-10 M b) 1.1 x 108 M c) 1.1 x 107 M d) 1.1 x 106 M e) 1.1 x 10$ M
Which of the following is the expression for the solubility product of Ba3(AsO4)2? Select one: O a. Ksp=[Ba²+j°[Aso,³ ? O b. Ksp=[3 x Ba²"]°12 x AsO, 1? O c. Ksp=3[Ba2+j3 + 2[AsO³]? O d. Kgp= [Ba3-1P[AsO1? O e. Kp=3[Ba²] × 2[AsOg³] Which one of the following cannot act as a buffer solution? Select one: O a. 1.0 M KF and 1.0 M HF rch F4 ES F7 F8 F9 F10 F11 F12 2$ & 4 7 9 R Y 1O F V B
Calculate the final molarity of H2O2H2O2 if 5.9 mL5.9 mL of a 3.0% w/w H2O23.0% w/w H2O2 solution, which has a density of 1.0 g/mL,1.0 g/mL, is added to 5.9 mL5.9 mL of a starch-iodide solution. final [H2O2]=[H2O2]= MM Calculate the final molarity of H2O2H2O2 if 1.6 mL1.6 mL of the 3.0% w/w H2O23.0% w/w H2O2 solution is diluted with 3.4 mL3.4 mL water, then added to 5.0 mL5.0 mL of a starch-iodide solution. final [H2O2]=[H2O2]= M
Determine if the reaction favors the reactants or the products.
Calculate +he molarity of a Solution that contains 4.759 df NacI dissolved in 45.0 mL Of SOLition?
Given the following equilibrium constants at 415°C, Naz 0(s) 2 Na(1)+02(9) K1 = 9 x 10-25 Na0(g) Na(1) + 02 (9) K2 = 2 x 10-5 NazO2(s) 2 Na(1) + O2 (g) NaO2 (s) = Na(1)+02(g) K3 = 5 x 10-29 KA = 8 x 10 14 determine the values for the equilibrium constants for the following reactions: a. Naz 0(s) +02 (g) Naz O2 (s) Equilibrium constant b. NaO(g) + Naz 0(s) Naz O2 (s) + Na(l) Equilibrium constant = c. 2 Na0(g) - Naz O2 (s) Equilibrium constant = (Hint: When reaction equations are added, the equilibrium expressions are multiplied.)
please help!! 0.0183 g SrF2 dissolved in 250 mL of water to generate a saturated solution at 25°C. What is the solubility product constant, Ksp? The molar mass of SrF2 is 125.67 g/mol.
Consider the reaction below. What is the effect on the concentration of acetic acid (CH3CO2H), water (H20) hydronium ion (H30*), and acetate ion (CH3CO2) if H3o is added to the reaction? CH3CO2H (aq) + H20 (1) = H30* (aq) + CH3CO2 (aq) Ka=1.8x10-5 The concentration of CH3CO2H The concentration of H30* The concentration of CH3CO2¯ The concentration of H2 increases decreases does not change