The following results were obtained by monitoring the reaction H*(ag) + l'(ag) + ½ H2O2(ag) → ½ I2(ag) + H2O [I] [H,O2] rate 0.020 0.020 3.3 x 10-5 0.040 0.020 6.6 x 105 0.060 0.020 9.0 x 105 0.040 0.040 1.3 x 10-4 Determine the order of the reaction with respect to I' and H2O2 and also determine the value for the rate constant, k

The following results were obtained by monitoring the reaction H*(ag) + l'(ag) + ½ H2O2(ag) → ½ I2(ag) + H2O [I] [H,O2] rate 0.020 0.020 3.3 x 10-5 0.040 0.020 6.6 x 105 0.060 0.020 9.0 x 105 0.040 0.040 1.3 x 10-4 Determine the order of the reaction with respect to I' and H2O2 and also determine the value for the rate constant, k

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

estion 3 of 3 Time and concentration data were collected for the reaction 0.52 A → products 0.48 0.44- t (s) [A] (M) 0. 0.52 0.40- 20 0.43 0.36- 40 0.35 0.32- 60 0.29 0.28 - 80 0.23 100 0.19 0.24 0.20. The blue curve is the plot of the data. The straight orange line is tangent to the blue curve at t = 40 s. 0.16. 0 10 20 30 40 50 60 70 80 90 t (s) Approximate the instantaneous rate of this reaction at time t = 40 s. instantaneous rate: M/s [A] (M)
Time and concentration data were collected for the reaction 0.52 A -> products 0.48 0.44 t(s) [A] (M) 0 0.52 0.40- 0.36 20 20 0.43 0.32 40 40 0.35 0.28 60 60 0.29 0.24 88 80 0.23 0.20. 0.16. 100 0.19 The blue curve is the plot of the data. The straight orange line is tangent to the blue curve at t = 40 s. Approximate the instantaneous rate of this reaction at time t = 40 s. instantaneous rate: M/s 0 10 20 30 40 50 60 70 80 90 100 t(s)
While creating the E3 reaction mixture, a student obtains the following data. Calculate the initial thiocyanate ion concentration, [SCN]o, in the reaction mixture in millimolar (mM. Give your answer to three decimal places. Fe(NO3)3 NaSCN 0.10 MHNO3 2.042 x 10-3 M 1.98 × 10-3M initial buret reading (mL) 0.02 0.03 0.05 final buret reading (mL) 5.09 2.33 2.93 Your Answer: Answer
Based on your ICE table (Part 2) and the definition of Ka, set up the expression for Ka in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Ka = 2.9 × 10-8 RESET [0] (0.13] [0.37] (0.010] [0.040] [0.10] [0.40] [x] [2x] [0.13 + x) [0.13-x] [0.010+x] [0.010-x] [0.040 + x] [0.040 - x] [0.10+x] [0.10-x] [0.40+x] [0.40-x] PREV 2 Based on your ICE table (Part 2) and the equilibrium expression for Ka (Part 3), determine the pH of solution. pH = RESET 0 7.3 × 10* 5.86 18.74 1.4 × 10+ 0.13 8.14 0.89
Question 20 of 20 Determine the activation energy for the redox reaction Q2* + 2 R3t → Q4* + 2 R2*. Rate Constant Temperature kJ/mol 3.12 x 103 M-1s-1 275 K 1 2.70 x 104 M-1s-1 300 K 6. C +/- 0. x 100 MacBook Pro DII DD 000 000 F11 F12 F9 F10 esc F7 F8 F4 F5 F6 F1 F2 F3 & ! # 2. 8. 7, %24
3. The following results were obtained by monitoring the reaction + 1e+1/2 H,Oo) 1/2 I(a0)+ H,O (bo) rate l'o'Hl 0.020 0.020 3.3 x 105 0.040 0.020 6.6 x 105 0.020 9.0 x 10-5 0.040 0.040 1.3 x 104 Determine the order of the reaction with respect to I' and H,O, and also determine the value for the rate constant, k
Using the mechanism below, what would be the appropriate equilibrium constant expression for the overall reaction? Step 1: H(aq) + H₂O2(aq) → H3O₂ (aq) Step 2: H3O₂ (aq) + Br (aq) → HOBr(aq) + H₂O(1) Step 3: HOBr(aq) + H*(aq) + Br (aq) ← → Br₂(aq) + H₂O(1) K= K= K = K= [Br₂] [H₂O]2 [H+]2[Br]2 [H₂O₂] [H+]2[Br]2 [H₂O₂] [Br₂] [Br₂] [H+][Br] [H₂O₂] [Br₂] [H+12[Br-12 [H₂O₂] fast slow fast
Complete the table below:
Based on your ICE table (Part 1) and the definition of Ka, set up the expression for Ka in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Ka = = 1.8 × 10-5 [500.0] [0.200] RESET [5.00] [1.0 × 10-9] [1.0 × 10-9] [1.8 × 10-5] [x + 5.00] [x + 1.0 × 10] [x-1.0 x 10 x + 1.0 × 10-] [x-1.0 × 10-] [x+1.8 × 10] [x-1.8 × 10%] [0] [x-5.00] < PREV 1 2 3 Based on your ICE table (Part 1) and the equilibrium expression, Ka (Part 2), determine the original mass of solid CH3COONa added to create this buffer solution. MNACH3COO g 0 0.360 30 21 43 11 15 36 x 10' 59 x 105 43 x 105 RESET 59 50
help please answer in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working