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) +...
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 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
For the decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C 2 H2O2(aq) 2 H2O(l) + O2(g) the following data have been obtained: 6.26x10-2 3.39x10-2 1.84x10-2 9.96x10-3 [H202], M time, min 9.28 18.6 27.9 The average rate of disappearance of H2O2 over the time period from t=18.6 min to t = 27.9 min is M min-1
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...
The gas phase decomposition of hydrogen peroxide at 400 °C H2O2(g)—>H2O(g) + 42 O2(g) is second order in H2O2. In one experiment, when the initial concentration of 1,02 was 0.153 M, the concentration of H2O2 dropped to 2.51x10-2 M after 36.1 seconds had passed. Based on these data, the rate constant for the reaction is M's-1 The gas phase decomposition of nitrogen dioxide at 383 °C NO2(g)—>NO(g) + 12 02(g) is second order in NO, with a rate constant of...
A) B) C) The decomposition of nitramide in aqueous solution at 25°C NH NO2(aq) → N2O(g) + H2O(1) is first order in NH, NO, with a rate constant of 4.70x10s. M after 46963 s If the initial concentration of NH NO2 is 0.646 M, the concentration of NHNO, will be have passed. Submit Answer Retry Entire Group 7 more group attempts remaining The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H,02(aq)->H2O(l) + 12 02(g) is first...
The gas phase decomposition of hydrogen peroxide at 400 °C H2O2() H2O(g) + %0,(8) is second order in H,O, with a rate constant of 0.650 M's! If the initial concentration of H20, is 0.204 M, the concentration of H,O, will be 3.59x10M after seconds have passed Submit Answer Retry Entire Group 4 more group attempts remaining
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.
Please show work I am not getting the correct answers 1. Hydrogen peroxide, H2O2, decomposes spontaneously through the following reaction. 2H2O2(aq) 2H2O(g) + O2(g) The kinetics are second order, and the half‐life is 17.3 min when a 1.75 M solution of H2O2 is made. What is the concentration of the solution after 24.8 min? 2. The decomposition of N2O5 occurs by the following reaction: 2N2O5(g) 4NO2(g) + O2(g) The rate constant is experimentally determined to be 3.4 x 10‐4 s‐1....