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LAB FINAL 1. The kinetics of the reaction 103- (aq) + 81' (aq) + 6H30+ (aq)...
Lab 1l: Kinetics In the Kinetics Lab, the reaction of iodide with persulfate was studied, and it ...
Lab 1l: Kinetics In the Kinetics Lab, the reaction of iodide with persulfate was studied, and it was determined that the rate law was first order in each reactant. 21(a)s20 (22 S042(ag) rateS2091 (a) If [I-] = 0.0550 M, [S2O82-]-0.0350 M, and kー0.00400 M-1 s-1, what is the reaction rate? M/s (b) If [I-]-0.0500 M, [S2082-]-0.0350 M, and the reaction rate is 5.90×10-6 M/s, what is the rate constant? M-1s-1 (c) The reaction rate was determined indirectly in this lab...
Calculate the value of Kc for the generic acid-base reaction: B (aq) + HA(aq) BH(aq) +...
Calculate the value of Kc for the generic acid-base reaction: B (aq) + HA(aq) BH(aq) + A-(aq) Kc = ? Given the following information B(aq) + H20 (1) BH(aq) + OH"(aq) Kb = 2.80 x 10-7 HA(aq) + H2O(1) = A*(aq) + H30+(aq) Kg = 1.00 x 10-5 2H2O(1) = H30+ (aq) + OH- (aq) Kw = 1.00 x 10-14 Calculate Kc for the following reaction: Ex-(aq) + HA(aq) = BH(aq) + F"(aq) Kc = ? Record your answer in...
Initial rate data are listed in the table for the reaction: NH4+ (aq) + NO2 (aq)...
Initial rate data are listed in the table for the reaction: NH4+ (aq) + NO2 (aq) → N2 (g) + H20 (1) AWNA Experiment (NH4+1: [NO2). Initial rate (M/s) 0.24 0.10 17.2 x 10-4 0.12 0.10 13.6 x 10-4 0.15 15.4 x 10-4 0.12 0.12 4.3 x 10-4 0.12 First determine the rate law and rate constant. Under the same initial conditions as in Experiment 4, calculate (NH4+] at 103 seconds after the start of the reaction. In this experiment,...
3. For the reaction 103 (aq) + 51(aq) + 6H*(aq) → 312(aq) + 3H2O(1) the rate...
3. For the reaction 103 (aq) + 51(aq) + 6H*(aq) → 312(aq) + 3H2O(1) the rate of disappearance of I (aq) at a particular time and concentration is 2.6 x 10-' mol/(L · s). What is the rate of appearance of 12(aq)? A) 4.3 10-' mol/(L •s) B) 7.8 x 10-3 mol/(L • s) C) -1.6 x 10 mol/(L • s) D) 1.6 x 10' mol/(L •s) E) 6.4 x 10^'mol/(L •s) 4. For the first-order reaction 1/2 N2O4(g) →...
Initial rate data are listed in the table for the reaction: NH4+ (aq) + NO2 (aq) + N2(g) + H20 (1) Experiment (NH4+) (N...
Initial rate data are listed in the table for the reaction: NH4+ (aq) + NO2 (aq) + N2(g) + H20 (1) Experiment (NH4+) (NO2). Initial rate (m/s) AWN + 0.24 0.10 0.12 0.10 0.120.15 0.12 0.12 7.2 x 10-4 3.6 x 104 5.4 x 10-4 4.3 x 10-4 First determine the rate law and rate constant. Under the same initial conditions as in Experiment 4, calculate [NH4+) at 114 seconds after the start of the reaction. In this experiment, both...
1) For the following reaction, which of the following is a conjugate acid-base pair? HC20(aq)+ H20)...
1) For the following reaction, which of the following is a conjugate acid-base pair? HC20(aq)+ H20) H:0 (aq) C0,(aq) a. HC20 and H20 b. H20 and C202 c. HC20 and H30 d. HCzOr and C20 2) The pH of a solution of hydrochloric acid is 1.5. What is the concentration of the acid? a. 0.22 mol/dm b. 0.32 mol/dm3 c. 3.2x 102 mol/dm d. 2.2x 10-3 mol/dm 3) Which of the following diagrams represents the acid with the highest pH?...
An iodine-clock kinetics experiment was performed by varying the composition of reactant solutions and measuring the...
An iodine-clock kinetics experiment was performed by varying the composition of reactant solutions and measuring the resulting rates of reaction. Initial Rate Experiment 1 Initial Rate Experiment 2 Initial Rate Experiment 3 Test tube contents 10.0 mL 0.10 M NaI(aq) 10.0 mL 0.10 M Na2S2O8(aq) 5.0 mL 0.0050 M Na2S2O3(aq) 1.0 mL starch solution 10.0 mL 0.10 M NaI(aq) 5.0 mL 0.10 M Na2S2O8(aq) 5.0 mL 0.10 M Na2SO4(aq) 5.0 mL 0.0050 M Na2S2O3(aq) 1.0 mL starch solution 5.0 mL...
The following data were collected for the reaction HSO, (aq) + Clo, (aq) → CIO, (aq)...
The following data were collected for the reaction HSO, (aq) + Clo, (aq) → CIO, (aq) + So, (aq) + H (aq), at 30 °C. -1 -1 Experiment No. -1-1 Rate, in mol LS [HSO, ], in mol L 0.05 [CIO, ), in mol L 0.010 1.2 x 10 12 0.10 0.010 2.3 x 10 5 3 0.20 0.020 9.5 x 10 What is the numerical value of the rate constant for the reaction? Select one: a. 0.48 -2 -3...
1) Determine the rate law and the rate constant given the data below. 2 MnO4 (aq)...
1) Determine the rate law and the rate constant given the data below. 2 MnO4 (aq) + 5 C103(aq) + 6 H+(ag) Experiment Mn04] 0.10 2 0.25 3 0.10 4 0.10 2 Mn2+ (aq) + 5 C104 (aq) + 3 H20 (1) [C103] [H] Initial Rate(M/s) 0.10 0.10 5.2 x 10-3 0.10 0.10 3.3 x 10-2 0.30 0.10 1.6 x 10-2 0.10 0.20 7.4 x 10-3
part 1 part 2 Consider the following reaction: 2 CO2(aq) + 2OH(aq) + C103"(aq) + CIO3...
part 1
part 2
Consider the following reaction: 2 CO2(aq) + 2OH(aq) + C103"(aq) + CIO3 (aq) + H2000 (a) The rate law for this reaction is second order in CO2(aq) and first order in OH(aq). What is the rate law for this reaction? Rate = k [CIO(aq)] [OH(aq)] Rate = k [CO2(aq)] [OH(aq)] Rate = k [CIO2(aq)] [OH(aq)]2 Rate - [CIO3(aq)] [OH(aq)]2 Ratek [CIO (aq)] [OH (9) Ratek [CIO2(aq)](OH(aq)] (b) If the rate constant for this reaction at a...
Lab 1l: Kinetics In the Kinetics Lab, the reaction of iodide with persulfate was studied, and it was determined that the rate law was first order in each reactant. 21(a)s20 (22 S042(ag) rateS2091 (a) If [I-] = 0.0550 M, [S2O82-]-0.0350 M, and kー0.00400 M-1 s-1, what is the reaction rate? M/s (b) If [I-]-0.0500 M, [S2082-]-0.0350 M, and the reaction rate is 5.90×10-6 M/s, what is the rate constant? M-1s-1 (c) The reaction rate was determined indirectly in this lab...
Calculate the value of Kc for the generic acid-base reaction: B (aq) + HA(aq) BH(aq) + A-(aq) Kc = ? Given the following information B(aq) + H20 (1) BH(aq) + OH"(aq) Kb = 2.80 x 10-7 HA(aq) + H2O(1) = A*(aq) + H30+(aq) Kg = 1.00 x 10-5 2H2O(1) = H30+ (aq) + OH- (aq) Kw = 1.00 x 10-14 Calculate Kc for the following reaction: Ex-(aq) + HA(aq) = BH(aq) + F"(aq) Kc = ? Record your answer in...
Initial rate data are listed in the table for the reaction: NH4+ (aq) + NO2 (aq) → N2 (g) + H20 (1) AWNA Experiment (NH4+1: [NO2). Initial rate (M/s) 0.24 0.10 17.2 x 10-4 0.12 0.10 13.6 x 10-4 0.15 15.4 x 10-4 0.12 0.12 4.3 x 10-4 0.12 First determine the rate law and rate constant. Under the same initial conditions as in Experiment 4, calculate (NH4+] at 103 seconds after the start of the reaction. In this experiment,...
3. For the reaction 103 (aq) + 51(aq) + 6H*(aq) → 312(aq) + 3H2O(1) the rate of disappearance of I (aq) at a particular time and concentration is 2.6 x 10-' mol/(L · s). What is the rate of appearance of 12(aq)? A) 4.3 10-' mol/(L •s) B) 7.8 x 10-3 mol/(L • s) C) -1.6 x 10 mol/(L • s) D) 1.6 x 10' mol/(L •s) E) 6.4 x 10^'mol/(L •s) 4. For the first-order reaction 1/2 N2O4(g) →...
Initial rate data are listed in the table for the reaction: NH4+ (aq) + NO2 (aq) + N2(g) + H20 (1) Experiment (NH4+) (NO2). Initial rate (m/s) AWN + 0.24 0.10 0.12 0.10 0.120.15 0.12 0.12 7.2 x 10-4 3.6 x 104 5.4 x 10-4 4.3 x 10-4 First determine the rate law and rate constant. Under the same initial conditions as in Experiment 4, calculate [NH4+) at 114 seconds after the start of the reaction. In this experiment, both...
1) For the following reaction, which of the following is a conjugate acid-base pair? HC20(aq)+ H20) H:0 (aq) C0,(aq) a. HC20 and H20 b. H20 and C202 c. HC20 and H30 d. HCzOr and C20 2) The pH of a solution of hydrochloric acid is 1.5. What is the concentration of the acid? a. 0.22 mol/dm b. 0.32 mol/dm3 c. 3.2x 102 mol/dm d. 2.2x 10-3 mol/dm 3) Which of the following diagrams represents the acid with the highest pH?...
The following data were collected for the reaction HSO, (aq) + Clo, (aq) → CIO, (aq) + So, (aq) + H (aq), at 30 °C. -1 -1 Experiment No. -1-1 Rate, in mol LS [HSO, ], in mol L 0.05 [CIO, ), in mol L 0.010 1.2 x 10 12 0.10 0.010 2.3 x 10 5 3 0.20 0.020 9.5 x 10 What is the numerical value of the rate constant for the reaction? Select one: a. 0.48 -2 -3...
1) Determine the rate law and the rate constant given the data below. 2 MnO4 (aq) + 5 C103(aq) + 6 H+(ag) Experiment Mn04] 0.10 2 0.25 3 0.10 4 0.10 2 Mn2+ (aq) + 5 C104 (aq) + 3 H20 (1) [C103] [H] Initial Rate(M/s) 0.10 0.10 5.2 x 10-3 0.10 0.10 3.3 x 10-2 0.30 0.10 1.6 x 10-2 0.10 0.20 7.4 x 10-3
part 1
part 2
Consider the following reaction: 2 CO2(aq) + 2OH(aq) + C103"(aq) + CIO3 (aq) + H2000 (a) The rate law for this reaction is second order in CO2(aq) and first order in OH(aq). What is the rate law for this reaction? Rate = k [CIO(aq)] [OH(aq)] Rate = k [CO2(aq)] [OH(aq)] Rate = k [CIO2(aq)] [OH(aq)]2 Rate - [CIO3(aq)] [OH(aq)]2 Ratek [CIO (aq)] [OH (9) Ratek [CIO2(aq)](OH(aq)] (b) If the rate constant for this reaction at a...
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