The reaction of hydrogen peroxide with iodine,
H2O2(aq)+I2(aq)?OH?(aq)+HIO(aq)
is first order in H2O2 and first order in I2 . If the concentration of H2O2 was increased by half and the concentration of I2 was quadrupled, by what factor would the reaction rate increase?
ate = k(H2O2)^1(I2)^1
assume H2O2 was 1 and I2 was 1. Rate would be k(1)(1) = 1
Now, H2O2 increased by half and quadruple I2.
Rate k(1.5)(4) = 6
The reaction of hydrogen peroxide with iodine, H2O2(aq)+I2(aq)?OH?(aq)+HIO(aq) is first order in H2O2 and first order...
1) The reaction of hydrogen peroxide with iodine, H2O2(aq)+I2(aq)⇌OH−(aq)+HIO(aq) is first order in H2O2 and first order in I2. If the concentration of H2O2 was increased by half and the concentration of I2 was quadrupled, by what factor would the reaction rate increase? 2) Consider the following reaction: O3(g)→O2(g)+O(g) Using the results of the Arrhenius analysis (Ea=93.1kJ/mol and A=4.36×1011M⋅s−1), predict the rate constant at 298 K . 3. The rate constant of a chemical reaction increased from 0.100 s−1 to...
26. Hydrogen peroxide decomposes into water and oxygen in a first-order process. H2O2(aq) → H2O(l) + 1/2 O2(g) 26. Hydrogen peroxide decomposes into water and oxygen in a first-order process. H2O2(aq) → H2O(2) + 1/2O2(g) At 20.0 °C, the half-life for the reaction is 3.05 x 104 seconds. If the initial concentration of hydrogen peroxide is 0.52 M, what is the concentration after 8.00 days?
1) Hydrogen peroxide, H2O2(aq), decomposes to H2O(l) and O2(g) in a reaction that is first order in H2O2 and has a rate constant k = 1.06×10−3 min−1 at a given temperature. How long will it take for 15% of a sample of H2O2 to decompose? 2)The decomposition of nitrogen dioxide, NO2, into nitrogen monoxide and oxygen at a high temperature is second-order in NO2. The rate constant for this reaction is 3.40 L/mol×min. Determine the time needed for the concentration...
Hydrogen peroxide (H2O2) decomposes as a first order reaction with a half-life of 17.2 minutes in the presence of a Fe(III) catalyst. How long would it take containing a 0.27 M H2O2 solution to become to a 0.027 M H2O2 solution after the Fe(III) catalyst is added?
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1a) The decomposition of hydrogen peroxide is first order in [H2O2]. After 60 min the [H2O2] has fallen from 3.7 M to 3.4 M. The rate constant k, in min-1 , is A. 1.4 X 10-3 B. 6.1 X 10-4 C. 2.7 X 10-2 D. 8.3 X 10-3 E. 1.2 x 10-2 1b) What is the half-life, in seconds, of a first order reaction if 30% of the reactant has decomposed in 50 seconds? A. 50 B. 83 C. 26...
The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H2O2(aq) ------> H2O(l) + ½ O2(g) is first order in H2O2 with a rate constant of 1.10×10-3min-1. If the initial concentration of H2O2 is 5.52×10-2 M, the concentration of H2O2 will be 1.56×10-2 M after _____ min have passed.
The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H2O2(aq)->H2O(1) + 12 02(g) is first order in H2O2- During one experiment it was found that when the initial concentration of 1,0, was 3.16x10-2 M, the concentration of H2O2 dropped to 8.09x10-3 M after 945 min had passed. Based on this experiment, the rate constant for the reaction is nin-1
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