The decomposition of nitramide in aqueous solution at 25 °C NH,NO2(aq)N20(g) + H2O(1) is first order in NH2NO2. During one experiment it was found that when the initial concentration of NH2NO2 was 0.402 M, the concentration of NH2NO2 dropped to 7.40×10-2 M after 25187 s had passed. Based on this experiment, the rate constant for the reaction is s-!

The gas phase decomposition of dinitrogen pentoxide at 335 K N205(g)2 NO2(g) + ½ 02(g) is first order in N205. During one experiment it was found that when the initial concentration of N205 was 7.50×10-2 M, the concentration of N205 dropped to 2.09×10-2M after 198 s had passed. Based on this experiment, the rate constant for the reaction is || IS s-1.

17. The following overall reaction has a second order rate law as determined by experiment: H₂(g) + 21C1(g) → 12(g) + 2HCl(g) Rate = k[H₂][ICI] Propose a mechanism that is consistent with the experimentally determined rate law.

The decomposition of nitramide in aqueous solution at 25 °C NH2NO2(aq)–N20(g) + H20(1) is first order in NH,NO2 with a rate constant of 0.0000470 s1. If the initial concentration of NH2NO2 is 0.548 M, the concentration of NH2NO2 will be 0.0986 M after s have passed.

In aqueous solution buffered at a pH of 6.75 Penicillin G (molecular weight of 334.39 g/mole) undergoes hydrolysis via a pseudo first order reaction that has an activation energy of 77.3 kJ/mole and a pseudo first order rate constant of 1.58 x 10-7 s-1 at 30°C. What is the half life (in days) of Penicillin G under the conditions described?

The recombination reaction2 HO2(g) → H2O2(g) + O2(g)has a second-order rate constant of 2E9 M-1 s-1. Calculate the half-life of the reaction if the initial concentration of HO2(g) is 2.58E-11 M.Note: the coefficient 2 in the reaction means that the integrated rate law for this reaction is:1/ct = 1/c0 + 2kt

Please don't provide handwritten solution ....

The decomposition of nitrous oxide at 565 °C N₂O(g) → N₂ (9)+½O₂(g) 1 is second order in N₂O with a rate constant of 1.10 × 10-³ M s If the initial concentration of N₂O is 2.16 M, the concentration of N₂O will be M after 1480 seconds have passed.

The gas phase decomposition of nitrosyl chloride at 400 K NOCI(g) NO(g) + ½ Cl½(g) is second order in NOCI with a rate constant of 5.90×10+ M's'. If the initial concentration of NOCI is 4.60×10 ² M, the concentration of NOCI will be 8.51x10 3M after seconds have passed.

The gas-phase reaction 2NO2Br →2NO2 + Br2 has r = k[NO2Br]. Devise a mechanism consistent with this rate law.