A first order gas phase reaction : A2B2(g) → 2A(g) + 2B(g) at the temperature 400°C has the rate constant k = 2.0 × 10-4 sec-1. What percentage of A2B2 is decomposed on heating for 900 seconds? (Antilog 0.0781 = 1.197)

The gas phase decomposition of dinitrogen pentoxide at 335 K 2 N205 →4 NO2+02 has the following relationship between rate and concentration, where the bracket around the formula indicates concentration and k is a constant called the rate constant. Rate = k[N2O5l %3D If the value of k is 7.38×10~$ s', what is the rate of the reaction when [N2O5] = 0.180 M? Ms-

The reaction 2 NO(g) + O2(g) --> 2 NO2(g) proceeds through the following mechanism:      2 NO(g) --> N2O2(g)N2O2(g) + O2(g) --> 2 NO2(g) (a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [NO] [O2] Rate = k [NO]2 [O2]     Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2   (b) What would the rate law be if the first step of this mechanism were rate-determining? Rate = k [NO] [O2] Rate = k [NO]2 [O2]     Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 Rate = k [NO]

The rate law for the reaction A2BM2(aq) + 2A(aq) + 2D(aq) → D2(aq) + 2A½Bm (aq) is rate = k(A2Bm2)(D). %3D What is the overall order of the reaction? O zeroth order O first order third order second order

Can you explain step by step?

The decomposition of nitramide in aqueous solution at 25 °CNH2NO2(aq)N2O(g) + H2O(l)is first order in NH2NO2.During one experiment it was found that when the initial concentration of NH2NO2 was 0.886 M, the concentration of NH2NO2 dropped to 0.103 M after 30353 s had passed.Based on this experiment, the rate constant for the reaction is s-1.

The reaction 2 NO(g) + O2(g) --> 2 NO2(g) proceeds through the following mechanism: 2 NO(g) --> N2O2(g)N2O2(g) + O2(g) --> 2 NO2(g) (a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [NO] [O2] Rate = k [NO]2 [O2]     Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 (b) What would the rate law be if the first step of this mechanism were rate-determining? Rate = k [NO] [O2] Rate = k [NO]2 [O2]     Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 Rate = k [NO]

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Q1: A very unstable molecule, 'XYZ', decomposes via the following set of first order reactions, XY+Z k₂ XYZ k₁ « k3 X + YZ X+Y+Z If the initial concentration of XYZ is [XYZ]o, show that the decomposition of XYZ follows, [XYZ] = [XYZ]o exp[-(k)+k₂+ k3)t] Q2: Radioactive decay is a first order kinetic process. A convenient source of gamma rays for radiation chemistry research is 60Co, which decays to give a beta particle, gamma rays and Ni. The half-life for the decay is 5.27 years. What is the rate constant for the decay process? How many days will it take for a sample of 60Co to decay to 1/8th of its original amount? Q3: Hydrogen peroxide, H₂O2, decomposes in water by a first order kinetic process. A solution of 0.156 mol/L H₂O2 in water has an initial decomposition rate of 1.14 x 105 mol L´¹s¹. Calculate the rate constant for the decomposition reaction and the half-life of the reaction. Q 4: The equilibrium constant for the reaction H+ (aq) + OH(aq) = H₂O () at 25 °C is 5.49 x 10¹5 L…

The following data were obtained for the reaction 2C102 (ag) + 20H (ag) → Cl0; (ag) + C102 (ag) + H,0(1) A[CIO2] where Rate = - At [C102]o (mol L) [OH ], (mol L) Initial Rate (molL·s) 0.0750 0.150 1.94 x 10-1 0.150 0.150 7.76 x 10-1 0.150 0.0750 3.88 x 10-1 a Determine the rate law. (Use k for the rate constant.) Rate = k[ClO,][OH] b Determine the value of the rate constant. Rate constant = 2.30x1 / L²/mol? - s c What would be the initial rate for an experiment with [CIO2], = 0.140 mol/L and [OH], = 0.0668 mol/L? Rate = mol/L·s