The following data was collected for the reaction: A + 2B + C arrow D +...
For the reaction 3A(g) + 2B(g) → 2C(g) + D(g) the following data was collected at constant temperature. Determine the correct rate law for this reaction. run [A] (M) [B] (M) Rate (M/s) 1 . 0.125 0.200 7.25 2 0.375 0.200 21.75 3 0.250 0.400 14.50
24. Initial rate data were obtained for the following reaction: A(g) + 2B(g) → C(g) + D(g) initial initial [Al, mol/L [B], mol/ initial rate Experiment 0.10 0.15 0.30 0.15 0.10 0.45 1.8 .9 0. 200 What are the rate law and k value for the reaction?
For the reaction 3A(g) + 2B(g) → 2C(g) + 2D(g) the following data was collected at constant temperature. Determine the correct rate law for this reaction and value of rate constant. Trial Initial [A] Initial [B] Initial Rate (mol/L) (mol/L) (mol/(L• min)) 1 0.200 0.200 1.20 × 10–1 2 0.200 0.100 6.00 × 10–2 3 0.100 0.200 3.00 × 10–2 Predict the rate of reaction for Trial #4 using the correct rate law and rate constant. 4 0.300 0.200 ?????????
For the reaction A + 2B → C + D, the rate law is found to be rate = k[A][B]. The following mechanism, is proposed to explain the reaction. l+B→C+D a) Show that the proposed mechanism is consistent with the stoichiometry of the reaction. b) Which step must be the rate determining step? c) What is "T" called? Ca ta y st
For the reaction 3A(g) + 2B(g) → 2C(g) + 2D(g) the following data was collected at constant temperature. Determine the correct rate law for this reaction. Trial Initial [A]mol/L Initial[B]mol/L Initial Rate 1 0.200 0.100 6.00*10^-2 2 0.100 0.100 1.50 *10^-2 3 0.200 0.200 1.20*10^-1 4 0.300 0.200 ???????? Predict the rate of the reaction for Trial #4
Done Problem 1. Consider the general reaction 2A+2B+C D+3E And answer the following questions using the data given in the table below. a) What is the reaction order with respect to each reactant? b) Calculate the rate constant c) write the rate law for this reaction. d) Express the rate in terms of changes in concentration with time for each of the components Initial Rate 1 0180:101 076 05 0.990 0.990 0.270 0.620 0.620 0050 0410 0.940 0.040
Done Problem...
The following data were collected for the reaction between hydrogen and nitric oxide at 700 C 2H2(g) + 2N0(g) →2H2O(g) + N2(g) Experiment initial rate lME.- 0.010 0.00S0 0.010 0.025 0.025 0.012 2.4x 104 12 10 060 x 10 a) What is the rate law for the reaction? b) Calculate the rate constant for the reaction c)Suggest a plausible mechanism that is consistent with the rate law. Assume that an oxygen atom is the intermediate (d) More careful studies of...
6. (20 pts) The data below were collected for the following reaction at 25 °C: NO2(g) + CO(g) ? NO(g) + CO2(g) [NO2Initial 0.100 M 0.200 M 0.200 M 0.400 M COJinitial 0.100 M 0.100 M 0.200 M 0.100 M Initial rate 0.0021 Ms 0.0082 Ms 0.0083 Ms 0.033 M s a. (8 pts) What is the rate law for this reaction? (in the form Rate k[NOJ'icoj) b. (6 pts) What is the value of K? (Be careful with units...
Based on the data below, calculate the rate constant, k, for the reaction A + 2B --> C + D, if the rate law is rate = k[A]2[B]0. Experiment [A] M [B] M Initial Rate (M / s) 1 0.110 0.150 0.145 2 0.220 0.150 0.581 3 0.220 0.450 0.581
The following data were collected in two studies of the reaction below. A + 2B → C + D Time(s) Experiment #1 [A] (M) Experiment #2 [A] (M) 0 10.0 x 10-2 10.0 x 10-2 20 6.67 x 10-2 5.00 x 10-2 40 5.00 x 10-2 3.33 x 10-2 60 4.00 x 10-2 2.50 x 10-2 80 3.33 x 10-2 2.00 x 10-2 100 2.86 x 10-2 1.67 x 10-2 120 2.50 x 10-2 1.43 x 10-2 In Experiment #1,...