The following kinetic data were obtained for the reaction A B
Time(t) (hrs) 0 2 4 6 10
[A] (M) 1.240 0.775 0.564 0.443 0.310
Determine the reaction order, the rate constant, and the time (t1/2) at which [A]= 1/2[A]o = 0.62M
b.) A biological molecule undergoes a reversible interconversion between its trans and cis forms with first-order reaction rate constants k1(forward) and k-1(reverse). the following kinetics results were obtained starting with 10mM of the pure trans form until equilibrium was achieved at t =
Time(t) (s) 0 2.00 600 1000
[trans] (mM) 10.0 6.71 3.42 2.16 1.38
Determine k1, k-1 and the equilibrium constant Keq from these data
The following kinetic data were obtained for the reaction A B Time(t) (hrs) 0 2 4...
The following data are obtained for the reaction A ? products: t = 0 min. [A] 0.250 M, t 4.22 min, [A 0.210 Mt 6.60 min, [Al 0.188 M; t-10.61 min, [A]-0.150 M; t-14.48 min, [A 0.114 M, t 18.00 min, [A] 0.083 M. What are the order of this reaction and its rate constant, k?
The following data were obtained for the concentration vs. time for a certain chemical reaction. Values were measured at 1.00 s intervals, beginning at 0.00 and ending at 20.00 s. Concentrations in mM are: 10.00, 6.91, 4.98,4.32, 3.55, 3.21, 2.61, 2.50, 2.22, 1.91, 1.80, 1.65, 1.52, 1.36, 1.42, 1.23, 1.20, 1.13, 1.09, 1.00, and 0.92. A. Decide whether the data best fits zero-order, first-order, or second-order rate kinetics. Make sure to calculate the rate coefficients (with units) for the reaction...
For the reaction of 2A ---> B + C, the following data are obtained for [A] as a function of time time (min) [A] (mol L-1) 0 0.80 8 0.60 24 0.35 40 0.20 a). Determine the order and the rate law of the reaction. (Hint: Consider the integrated rate laws shown on the first page). b). Calculate the value of the rate constant k
PRACTICE EXAMPLE B: The following data are obtained for the reaction = 0.210 M: products: !=0 min, [A] 0.250 M; t 422 min, A 0.188 M, 10.61 min. A]0.150 M; t = A 14.48 min, : = 6.60 min, A (A] 0.114 M; i reaction and its rate constant, k? 18.00 min, [A] 0.083 M. What are the order of this Homework PRACTICE EXAMPLE A: In the decomposition reaction B following data are obtained: t Os, [B = 0.88 M;f...
B1. The following experimental data were obtained for the following reaction at 1000 K: 2 NO(g) + O2(g) 2 NO2(g) NOI (mol L OJ (mol L- Inital rate of reaction (mol L-'s - 0.0100 0.0200 0.0300 0.0200 0.0500 0.0200 3.02 x 10-5 3.02 x 10-4 2.72 x 10-4 (a) Determine the order of the reaction for each reactant (b) Determine the overall order of the reaction. Answer: (c) Calculate the rate constant at this temperature.
For the reaction below, the following data were obtained at constant temperature. Reaction: A(g) + B(g) + C(g) D(g) Exp't Initial [A] (mol/L) Initial [B] (mol/L) Initial [C] (mol/L) Initial Rate (mol/Ls) 1 0.0100 0.1500 0.0200 1.24 10-2 2 0.0200 0.1500 0.0200 2.48 10-2 3 0.0200 0.3000 0.0200 9.90 10-2 4 0.0100 0.1500 0.0400 1.24 10-2 (a) What is the order with respect to each reactant? with respect to [A]. with respect to [B]. with respect to [C]. (b) Select...
1: Consider the following set of data ccollected for a reaction of the form A --> products. time (seconds) [A] (M) 0 1.000 10 0.641 20 0.472 30 0.373 40 0.309 50 0.263 A: What is the average rate of the reaction for the first 10 seconds? rate = ___ M/s B: What is the average rate of the reaction between 30 and 40 seconds? rate = ___ M/s 2: Consider the dimerization of C4H6: 2 C4H6 --> C8H12 for...
For the overall reaction A+B+C products the following initial rate data were obtained: Rate, mol L-'s-1 Experiment # [A] [B]. [C]. 0.200 0.200 0.200 0.300 0.200 0.200 0.200 0.400 0.200 0.300 0.200 0.400 How many of the following statements are correct? 2.00 2.83 4.00 1) the reaction is first order in A 2) the overall reaction is second order 3) the rate of the reaction is proportional to [B]"2 4) the value of the specific rate constant, k, is 50.0...
41 The following data was experimentally obtained for the reaction: 2 of 2 (CH3)3CBr + H2O → (CH3)3COH + HBr t(h) (CH3)2CBr (mol/L) 0 10.39 x 102 3.15 8.96 x 102 6.20 7.76 x 102 10 6.39 x 102 18.30 3.53 x 102 30.80 2.07 x 102 a) Make the appropriate graphs and from them determine the order of reaction in relation to (CH3),CBr. In other words, the rate law expression will be like: Rate = k [(CH3)3CBr]" By concluding...
|References For the reaction N2(8) 2 H,0(8) 2 NO(g) +2 H3 (g) at 1100° C, the following data have been obtained. NO 4Na1/At rate |(mal t-) (mol L) (mol-L 5.93 x 10 0.380 0.0200 1.19 x 10 0.380 0.0807 1.19 x 10 0.760 0.161 Derive a rate law for the reaction. (Rate expressions take the general form rate k H Cl rate Determine the value of the rate constant. (in L mols) le L-mols Submit Answer Try Another Version 5...