For the reaction A +B+ C→D+ E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: [A] [B] [C) Initial rate Trial (М) (М) | (М) (M/s) 0.30 0.30 0.30 9.0×10-5 0.30 0.30 0.90 2.7×10¬4 0.60 0.30 0.30 3.6×10¬4 0.60 0.60 0.30 3.6×10¬4 1, 2. 3. 4.

Determine the rate law and the value of k for the following reaction using the data provided. 2 N205(g) 4 NO2(8) + O2(8) N205h (M) Initial Rate (M/s) 0.093 4.84 x 10-4 0.174 9.05 x 10-4 0.224 1.16 x 10-3 Rate = 6.0 x 10-1 M-25-1[N20513 Rate = 1.6 x 10-3 M1/25-1[N205]1/2 Rate = 5.2 x 10-3 s[N205] Rate = 1.7 x 10-2 M1/2s-1[N205]3/2 Rate = 5.6 x 10-2 M-151IN20512

A chemist runs a reaction at 25.0 C and determines that the reaction proceeds far too slowly. She decides that the reaction needs to speed up by a factor of 16. At what temperature should she run the reaction?

Consider the following elementary reaction: (g) (g) Suppose we let stand for the rate constant of this reaction, and stand for the rate constant of the reverse reaction. Write an expression that gives the equilibrium concentration of in terms of , , and the equilibrium concentration of .

The rate constant for the reaction H2(g) + I2(g) → 2HI(g) is equal to 2.40 M–1 s–1 at 355 ºC and 9.80 M–1 s–1 at 385 ºC. Using these results, estimated the value of the rate constant at 415 ºC.

Consider the following mechanism  in aqueous solutions. At 298 K the equilibrium constant for the first step is 5.75⋅10−35.75⋅10-3                                                                           k1k1                                Step1:              A + A         −−→←−−←→           A + B                                                                                               k−1k-1                                                                                             k2k2                                Step2:                   B       →→          P     When [A]  is large,  the second step is slow and the first step is fast and at equilibrium.    Under these conditions the following experimental data is gathered.   The third column in the table is a check to make sure [A] is sufficiently large. The ratio should be greater than 100 when the absolute uncertainties are ±0.01±0.01    Note that as time goes on here, the assumption we are making will not work.   Time…

Determine the rate law and the value of k for the following reaction using the data provided. CO(g) + Cl2(g) COC(g) [CO]; (M) [Cl2]; initial rate (M 1s1) 0.25 0.40 0.696 0.25 0.80 1.97 0.50 0.80 3.94 O Rate = 11 Ms [CO][Cl2]} Rate 36 M-1.8 5-1 [CO][Cl2]²8 || O Rate = 17 M-²s-' [CO][Cl2]² -1 O Rate = 4.4 MT|CO][Cl½]? M7s- [CO][Cl2]? S -3 O Rate = 18 M5-|co){{Cl2]} S

8. For the equilibrium between dinitrogen tetroxide and nitrogen dioxide: N₂O4 = 2 NO₂ Suppose that both the forward and reverse reactions are elementary processes with rate constants of kf, and k, respectively, and the equilibrium constant for the process is 14.48 at 298 K. If the rate of the reverse reaction is 1324 M/s when [NO₂] = 0.60 M, what is the half-life for the decomposition of dinitrogen tetroxide (the forward reaction) at the same temperature?

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What is the steady-state approximation? When is the steady state approximation a good approximation?