Given the data from below, fill up the missing data:Table 3.1. The different runs for the effect of persulfate and iodideconcentrations on reaction rate.RunRunª126345Beaker A0.2 M KI 0.2 M KCl, mL 0.1 MK₂S₂O810.00.05.05.02.57.55.05.05.05.0Beaker B (+ 3 drops of fresh starch)5.05.05.07.510.0[S208²-], M [I], Ma Condition: room temperaturebwill be referred to as set 1 of run 2 (two more sets will be prepared in Part C)Reactiontime in s48.1012a105.203233.10Reaction order with respect to [S₂08²-] rounded to the nearestintegerReaction order with respect to [I-] rounded to the nearestinteger0.1 MK₂SO 4.0 mM Na₂S₂O35.05.05.02.50.0[S203²-], M5.05.05.05.05.0Rate, M s-1RateConstant Laboratory Class # 4 (Chemical Kinetics):The rate of 1₂ formation will be measured to describe the rate of reaction. The I₂ formed from theS₂0²1 reaction is reduced back to I-byS₂03 ions.2S₂0² + I2 → S40²¯ +21¯Solutions:OOOOOO0.25L 0.2M KI0.25L 0.2M KCI0.25L 0.1M K₂SO80.25L 0.1M K₂SO40.25L 4.0mm Naz S2 03 - from Na2 S2 03 5H₂00.05L 0.01M CuSO40.02L of 1% (w/v) fresh starch solution (Moisten 0.20g of soluble starch with small amountof H₂O until a smooth paste is obtained. Pour slowly into 0.02L of boiling water.)

Total volume after the mixing of beaker-A and B in each Run = 10.0 mL + 0 mL + 5.0 mL + 5.0 mL + 5.0…

Given the data from below, fill up the missing data: Table 3.1. The different runs for the effect of persulfate and iodide concentrations on reaction rate. Run Runª 1 26 3 4 5 Beaker A 0.2 M KI 0.2 M KCl, mL 0.1 MK₂S₂O8 10.0 5.0 2.5 5.0 5.0 0.0 5.0 7.5 5.0 5.0 Beaker B (+ 3 drops of fresh starch) 5.0 5.0 5.0 7.5 10.0 [S208²-], M [I], M 0.1 M K₂SO4 4.0 mM Na₂S₂O3 a Condition: room temperature b will be referred to as set 1 of run 2 (two more sets will be prepared in Part C) Reaction time in s 48.10 1 2a 105.20 3 233.10 Reaction order with respect to [S₂08²-] rounded to the nearest integer Reaction order with respect to [I-] rounded to the nearest integer 5.0 5.0 5.0 2.5 0.0 [S203²-], M 5.0 5.0 5.0 5.0 5.0 Rate, M s-1 Rate Constant

Given the data from below, fill up the missing data: Table 3.1. The different runs for the effect of persulfate and iodide concentrations on reaction rate. Run Runª 1 26 3 4 5 Beaker A 0.2 M KI 0.2 M KCl, mL 0.1 MK₂S₂O8 10.0 5.0 2.5 5.0 5.0 0.0 5.0 7.5 5.0 5.0 Beaker B (+ 3 drops of fresh starch) 5.0 5.0 5.0 7.5 10.0 [S208²-], M [I], M 0.1 M K₂SO4 4.0 mM Na₂S₂O3 a Condition: room temperature b will be referred to as set 1 of run 2 (two more sets will be prepared in Part C) Reaction time in s 48.10 1 2a 105.20 3 233.10 Reaction order with respect to [S₂08²-] rounded to the nearest integer Reaction order with respect to [I-] rounded to the nearest integer 5.0 5.0 5.0 2.5 0.0 [S203²-], M 5.0 5.0 5.0 5.0 5.0 Rate, M s-1 Rate Constant

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

Consider the exothermic reaction: C2H4(g) + I2(g) = C2H412(g) In trying to maximize the amount of C2H412 produced, which of the following will not work? Assume that the reaction mixture reaches equilibrium. O increasing the temperature O decreasing the volume of the reaction vessel O increasing the amount of C2H4 O adding more l2
⦁ 4. Make your own energy diagram for an exothermic reaction that does not include a catalyst and one with a catalyst (Be sure each line is a different color or labeled). Label the axis of the diagram. Then, state what a catalyst is and how a catalyst affects the reaction rate.
Match each label in diagrams 1 and 2 (a-i) with the appropriate description. Each answer choice is used only once OR not at all. ΔH > 0 activation energy product exothermic reaction activated complex 1. a 2. b 3. c 4. d 5. e 6. f 7. g 8. h 9. i
Shown below is a concentration vs. time plot for the reaction A E B. For this reaction the value of the equilibrium constant is 0.100 0.080 0.060 B 0.040 A 0.020 0.000 0.00 1.00 2.000 3.00 4.00 5.00 Time (min) O Kc is less than 1. O Kc is equal to 1. O Kc is greater than 1. O Kc is equal to zero. Concentration (M)
What is the correct equilibrium constant expression for the balanced reaction shown below? PC13 (9) + PBr3 (9) PCl2Br (g) + PCIBr2(g) [PCl3] [PBr3] [PCl₂ Br][PCIBr₂] [PCIBr₂][PCl₂Br] [PCl3] [PBr3] [PCIBr₂][PCl3][PBr3] [PCl₂Br] [PCIBr₂]²[PCl₂Br]² [PCl3] [PBr3] [PCl3][PBr3] [PCIBr₂]²[PCl₂ Br]² O a. a O b.b OC.C O d.d O e.e a b C d e
QUESTION 12 Which statement correctly identifies a feature of the reaction mechanism shown in the diagram below? E (1) (7) (3) A. intermediates are only (3) and (4) B. intermediate is only (3) (5) C. intermediate is only (4) D. intermediates are only (5), (6) and (7) E. intermediates are only (7) and (6) (4) reaction progress (6) (2)
Consider the following general reaction for which gases A and B are mixed.in a constant volume container: A(g) + B(g) -> C(g) + D(g) According to collision theory, what happens to the rate of the reaction under the following changes: (consider each change separately) increase the temperature decrease the temperature increase the volume there is no change to the reaction rate A. decrease the volume the reaction rate increases В. decrease the pressure the reaction rate decreases C. collision theory does not allow you to predict the change in reaction rate increase the pressure D. decrease the concentration increase the concentration
Part A Consider the following reaction in chemical equilibrium: COC1₂ (g) CO(g) +Cl₂ (g) What is the effect of adding additional CO(g) to the reaction mixture? What is the effect of adding additional COC12 (g)? Match the words in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before submitting your answer. Submit right Cl₂ CO left COC12 Request Answer < Return to Assignment Adding COC2 increases the concentration of progress to shift to the Adding CO increases the concentration of to shift to the (away from the Provide Feedback " " |). Reset causing the reaction Help causing the reaction progress
At 40^0c, H202 (aq) will decompose according to the foll. reaction: 2 H202 (aq) ----2H20(l) +02 (g) The foll. data were collected for the concentration of h202 at various times. Time. [H202] (mol/L) 0. 1.600 3.10*10^4 0.592 6.20*10^4. 0.219 (a) Calculate the average rate of decomposition in H202 between0 and 3.10 * 10^4 s. use this rate to calculate the average rate of production 02 (g) over the same time period. (b) What are these rates for the time period 3.10*10^4 s. to 6.20 *10^4 s.? Rate of H202 decomposition Rate of O2 Production
400 300 + energy 200 - (kJ/mol) с +D 100 A + В reaction coordinate Use the energy diagram to answer these questions. I KJ/mol What is the heat of reaction? Exothermic Is the reaction exothermic or endothermic? Endothermic Neither Yes, it's kJ/mol Can you determine the activation energy? No. Can you determine the activation energy of the reverse reaction? Yes, it's kJ/mol С+D- A+B No.
When a chemical reaction is at equilibrium, the forward and reverse reactions occur at the same rate The concentrations of the different compounds in the reactions will remain constant. The relationship between the concentrations of the reactants and products is expressed as the equilibrium constant, Ke Drag each item to the appropriate bin. ▸View Available Hint(s) [0₂] Numerator Submit [H₂O]² [HC] [HCI] [Cl₂] Denominator 10₂1² [H₂O] Not used Reset Help [Cl₂1²
Which of the following will lower the activation energy for a reaction? Group of answer choices raising the temperature of the reaction. increasing the concentrations of reactants. increasing the surface area of the reactants. adding a suitable catalyst.