Rate of the reaction = ∆[I2]/∆t = [S2O32-]/(2×∆t) = 0.0001/(2×35.6) = 1.4045×10-6
= k ×[I-][H+][BrO3-] = k × 0.002 × 0.008×0.02
k = 1.4045×10-6/(0.002×0.008×0.02)
= 4.389
k = 4.4 M-2s-1 (Answer)
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ln(k2/k1) = Ea/R ( 1/T1 - 1/T2)
ln(2.5) = Ea/8.314 × (1/293.15 - 1/306.15)
Ea = 52592.54J/mol
= 52.592 kJ/mol
= 52.6 kJ/mol. (Answer)
If the rate law for the clock reaction is: Rate = k [1] [BrO3 ] [H]...
The reaction shown below has the rate law: Rate = k[BrO3-][Br-][H+]^2. BrO3-(aq) + 5 Br-(aq) + 6 H+(aq) → 3 Br2(aq) + 3 H2O(l) What is the order of reaction with respect to Br - ?
answer the questions Experiment 1084-04: lodine Clock Reaction Purpose Determine the rate law for an iodine clock reaction and study the influence of st on that reaction abruptly that it can be as startling as the sudden sound of an alarm clock, hence the clock reaction Background Information chemical equations can be written for chemical reactions, only some will proceed while others do not. Among the ones that do proceed some reactions occur as soon as reactants are mixed, while...
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1 7. The initial rate of the reaction: BrOz (aq) + 5 Br(aq) + 8 H+(aq) + 3 Brz(1) + H2O(1) Has been measured at the reactant concentrations shown (in mol/L) Experiment [Br03-] [Br] [H] Initial rate (mol/(L:s)) 0.10 0.10 0.10 8.0 x 10-4 2 0.20 0.10 0.10 1.6 x 10-3 3 0.10 0.20 0.10 1.6 x 10-3 4 0.10 0.10 0.20 3.2 x 10-3 a) what is the rate law expression and the rate constant k? [3] b) what...
1) You conduct a Vitamin C Clock Reaction at 298 K using the following initial concentrations: Concentration of Vitamin C = 0.0023 M Concentration of Iodide = 0.032 M Concentration of Hydrogen Peroxide = 0.18 M If the reaction time is 27 seconds, please calculate the reaction rate 6.7 x 10-3 M∙s–1 1.2 x 10-3 M∙s–1 4.9 x 10-7 M∙s–1 8.5 x 10-5 M∙s–1 2) You determine that x = 1 and y = 1 for the rate law of...
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Four experiments were conducted to discover how the initial rate of consumption of BrO3- ions in the reaction BrO3-(aq) + 5Br-(aq) + 6H+(aq) à 3Br2(aq) + 3H2O(l) varies as the concentration of the reactants are changed. Use the data given below to determine the average rate constant and write the rate law for this reaction. Experiment [BrO3-] (M) [Br-] (M) [H+] (M) Initial rate (M/s) 1 0.10 0.10 0.10 0.0012 2 0.20 0.10 0.10 0.0024 3 0.10 0.30 0.10 0.0035...
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