1. Consider the following kinetic data for the reaction: S206?(aq) + 31 (aq) → 2S0, (aq) + la (aq) [S:Og?] (mol/L) Expt # [1] (mol/L) Initial Rate, (mol/(L.s) 0.038 0.076 0.038 0.060 1.5 x 105 2.8 x 105 2.9 x 105 1 0.060 0.120 3 (a) Calculate the rate order w.r.t. each reactant and write the rate law for this reaction. (b) Calculate the rate constant and the reaction rate when the concentration of both reactants is 0.050 mol/L? 2. Kinetic data for the following reaction are summarized below. H2Q2(aq) + 31(aq) + 2H*(aq) → l3 (aq) + 2H20(), Expt # [H2O2] (mol/L) [1] (mol/L) [H*] Initial Rate (mol/L) mol/(L.s) 1 2 3 4 0.010 0.020 0.010 0.010 0.010 0.020 0.00050 0.00050 0.00050 0.00100 1.15 x 106 2.30 x 106 2.35 x 106 1.14 x 106 0.010 0.010 Determine the rate order with respect to each reactant and derive the rate law, expressed as: Rate = k[H2O2]"[I]^[H*J°. Calculate the rate constant, k.
1. Consider the following kinetic data for the reaction: S206?(aq) + 31 (aq) → 2S0, (aq) + la (aq) [S:Og?] (mol/L) Expt # [1] (mol/L) Initial Rate, (mol/(L.s) 0.038 0.076 0.038 0.060 1.5 x 105 2.8 x 105 2.9 x 105 1 0.060 0.120 3 (a) Calculate the rate order w.r.t. each reactant and write the rate law for this reaction. (b) Calculate the rate constant and the reaction rate when the concentration of both reactants is 0.050 mol/L? 2. Kinetic data for the following reaction are summarized below. H2Q2(aq) + 31(aq) + 2H*(aq) → l3 (aq) + 2H20(), Expt # [H2O2] (mol/L) [1] (mol/L) [H*] Initial Rate (mol/L) mol/(L.s) 1 2 3 4 0.010 0.020 0.010 0.010 0.010 0.020 0.00050 0.00050 0.00050 0.00100 1.15 x 106 2.30 x 106 2.35 x 106 1.14 x 106 0.010 0.010 Determine the rate order with respect to each reactant and derive the rate law, expressed as: Rate = k[H2O2]"[I]^[H*J°. Calculate 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...
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![1. Consider the following kinetic data for the reaction:
S206?(aq) + 31 (aq) → 2S0, (aq) + la (aq)
Expt #
[1]
(mol/L)
Initial Rate,
(mol/L)
(mol/(L.s)
0.038
0.076
0.038
0.060
1.5 x 105
2.8 x 105
2.9 x 105
1
0.060
0.120
3
(a) Calculate the rate order w.r.t. each reactant and write the rate law for this reaction.
(b) Calculate the rate constant and the reaction rate when the concentration of both reactants is 0.050
mol/L?
2. Kinetic data for the following reaction are summarized below.
H2Q2(aq) + 31(aq) + 2H*(aq) → l3 (aq) + 2H20(),
Expt # [H2O2]
(mol/L)
[1]
(mol/L)
[H*]
Initial Rate
(mol/L)
mol/(L.s)
1
2
3
4
0.010
0.020
0.010
0.010
0.010
0.010
0.020
0.00050
0.00050
0.00050
0.00100
1.15 x 106
2.30 x 106
2.35 x 106
1.14 x 106
0.010
Determine the rate order with respect to each reactant and derive the rate law, expressed as:
Rate = k[H2O2]™[I][H*]P. Calculate the rate constant, k.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F113fa95f-b0c0-4b06-8140-ddecc6eb5d11%2F45cb480f-b1f5-4948-8187-e6c8dab7e1d2%2F1nh6i7n_processed.png&w=3840&q=75)
Transcribed Image Text:1. Consider the following kinetic data for the reaction:
S206?(aq) + 31 (aq) → 2S0, (aq) + la (aq)
Expt #
[1]
(mol/L)
Initial Rate,
(mol/L)
(mol/(L.s)
0.038
0.076
0.038
0.060
1.5 x 105
2.8 x 105
2.9 x 105
1
0.060
0.120
3
(a) Calculate the rate order w.r.t. each reactant and write the rate law for this reaction.
(b) Calculate the rate constant and the reaction rate when the concentration of both reactants is 0.050
mol/L?
2. Kinetic data for the following reaction are summarized below.
H2Q2(aq) + 31(aq) + 2H*(aq) → l3 (aq) + 2H20(),
Expt # [H2O2]
(mol/L)
[1]
(mol/L)
[H*]
Initial Rate
(mol/L)
mol/(L.s)
1
2
3
4
0.010
0.020
0.010
0.010
0.010
0.010
0.020
0.00050
0.00050
0.00050
0.00100
1.15 x 106
2.30 x 106
2.35 x 106
1.14 x 106
0.010
Determine the rate order with respect to each reactant and derive the rate law, expressed as:
Rate = k[H2O2]™[I][H*]P. Calculate the rate constant, k.
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