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 D. 30 E. 97
1a) The decomposition of hydrogen peroxide is first order in [H2O2]. After 60 min the [H2O2]...
13. A. The decomposition of hydrogen peroxide is a first-order process with a rate constant of 1.06 x 10 min. How long will it take for the concentration of H2O2 to drop from 0.0200 M to 0.0120 M? <1 min 7.55 min 481 min 4550 min 31 400 min The rate constant is 5.4 C. D. E
The decomposition of hydrogen peroxide, H2O2, is first order with a rate constant, k=3.66 x 10-3s-1. If the initial concentration of H2O2 is 1.05M. Calculate the [H2O2] after 167s.
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(l) + ½ O2(g) is first order in H2O2 with a rate constant of 1.10×10-3 min-1. If the initial concentration of H2O2 is 5.66×10-2 M, the concentration of H2O2 will be 9.34×10-3 M after _______ min have passed.
The decomposition of hydrogen peroxide at 200 °C involves a first order rate law. The starting concentration of H202 is 0.20 M and changes to 0.0050 M after 10 minutes. Calculate the rate constant (in s1). 2H202(aq) 2H20(I) + 02(g) Select one: a. 4.0x 10-3 b. 4.0x 10-4 c. 6.1 x 103 d. 6.1 x 10-2 e. 4.0 x 10-2
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...
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?
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
In a study of the gas phase decomposition of hydrogen peroxide at 400 °C H2O2(g)----->H2O(g) + ½ O2(g) the concentration of H2O2 was followed as a function of time. It was found that a graph of 1/[H2O2] versus time in seconds gave a straight line with a slope of 0.884 M-1 s-1 and a y-intercept of 7.04 M-1. Based on this plot, the reaction is _______zerofirstsecond order in H2O2 and the rate constant for the reaction is M-1 s-1.
Saved Help Save & E The decomposition of hydrogen peroxide is a first-order process with a rate constant of 106 x 10- 3 min-1 How long will it take for the concentration of H202 to drop from 0.0200 M to 0.0120 M? 481 min 7.55 min <1 min Saved Hydrogen bromide will dissociate into hydrogen and bromine gases. 2HBr(g) = H2(g) + Br2(9) AH rxn = 68 kJ What effect will a temperature increase of 50°C have on this system...