The following data are for the decomposition of nitramide in aqueous solution at 25 °C. NH,NO2(aq) – N20(g) + H20(I) [ NH2NO2 ], 0.802 0.401 0.201 0.101 M time, min 175 350 525 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is min . (2) Based on these data, the rate constant for this O order reaction is min -1.

Given the following kinetic data for the first order production of H2O2, what is the rate constant (k) for the reaction? Do not put units in your answer. Trial Time (h) [H2O2] (M) ln[H2O2] 1 0 1.000 0.0 2 6.00 0.500 −0.693 3 12.00 0.250 −1.386 4 18.00 0.125 −2.079 5 24.00 0.0625 −2.772   Answer with steps please

The following data are for the decomposition of dinitrogen pentoxide in carbon tetrachloride solution at 30 °C. N₂O5 →→→→→2 NO₂ + ½ 02 [N₂05 ], M 0.200 0.100 5.00×10-2 time, min 0 133 266 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is 133 (2) Based on these data, the rate constant for this reaction is min -1 min. order 2.50×10-2 399

Which of the following is correct? (A) The activation energy changes when temperature changes. (B) The Arrhenius equation only applies to 1st order reactions. (C) The rate constants at higher temperatures are ALWAYS larger than at low temperatures for the same chemical reaction. (D) The rates of reaction at higher temperatures are ALWAYS larger than at low temperatures for the same chemical reaction.

the data in the table below were obtained for the reaction (see image) what is the magnitude of the rate constant for the reaaction

Ozone in the stratosphere can be depleted in catalyzed reactions. The overall reaction for this exothermic process is given by: O3 +O→2O2, via the mechanism: NO+O3 →NO2 +O2 NO2 +O→NO+O2 Is this mechanism a chain reaction? Why or why not? Identify both the catalyst and the reactive intermediate in this mechanism. Draw to a relative scale the potential energy vs. reaction coordinate diagram for both the uncatalyzed reaction and the catalyzed reaction. Label transition states, activation energy, and reactive intermediates where appropriate.

The following data are for the decomposition of dinitrogen pentoxide in carbon tetrachloride solution at 30 °C. N2O5- →2 NO2 + ½ 02 [N205 ], M 1.04 0.520 0.260 0.130 time, min 114 228 342 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is min . (2) Based on these data, the rate constant for thị -1 order reaction is min . zero first second

Given the following kinetic data for the first order production of H2O2, what is the rate constant (k) for the reaction? Do not put units in your answer. Trial Time (h) [H2O2] (M) ln[H2O2] 1 0 1.000 0.0 2 6.00 0.500 −0.693 3 12.00 0.250 −1.386 4 18.00 0.125 −2.079 5 24.00 0.0625 −2.772

You determine through experimentation that the reaction A⟶P is first order with respect to A. If the rate constant of the reaction is determined to be 5.58 x 108 s−1, what is the half-life when [A]= 0.352 M at 25 ∘C. τ1/2 in seconds

The decomposition of nitramide in aqueous solution at 25 °C NH₂ NO₂ (aq) → N₂O(g)+ H₂O(1) is first order in NH₂ NO2 with a rate constant of -1 4.70 × 10-5 S-¹ If the initial concentration of NH₂NO2 is 0.864 M, the concentration of NH₂ NO2 will be M after 32118 s have passed.