5. The following data was obtained from the reaction: NH:* (аq) + NO (ад) —> N2(g) + 2H>0() Initial Concentration (mol/L) Initial rate (mol/Ls) NO2- NH4+ 0.010 0.020 5.4 x 10-7 0.020 0.020 10.8 x 10-7 0.040 0.020 21.6 x 10-7 0.020 0.0202 10.8 x 10-7 0.020 0.0404 21.6 x 10-7 0.020 0.0606 32.4 х 10-7 (a) Determine the rate law. (b) Calculate the rate constant. (c) Calculate the initial rate, if [NO2] = 0.1 M and [NH4*] = 0.1 M

5. The following data was obtained from the reaction: NH:* (аq) + NO (ад) —> N2(g) + 2H>0() Initial Concentration (mol/L) Initial rate (mol/Ls) NO2- NH4+ 0.010 0.020 5.4 x 10-7 0.020 0.020 10.8 x 10-7 0.040 0.020 21.6 x 10-7 0.020 0.0202 10.8 x 10-7 0.020 0.0404 21.6 x 10-7 0.020 0.0606 32.4 х 10-7 (a) Determine the rate law. (b) Calculate the rate constant. (c) Calculate the initial rate, if [NO2] = 0.1 M and [NH4*] = 0.1 M

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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What is the concentration of A after 15.5 minutes for the reaction A → Products when the initial concentration of A is 0.750 M? (k = 0.0451 M-¹min-¹)
> A Moving to another question will save this response. estion 19 Consider the reaction in aqueous solution: 3r + S20g2- → 13 + 2 SO42- Under a given set of conditions, the concentration of 13 changes from 0,0 M to 7,6 x 10-4 M in 20 seconds. Calculate A[SO2yAt (in mol/L-s) for this time interval. O -6.5 x 10-5 mol/L-s O 5.0 x 10-5 mol/L·s O 1.2 x 10-5 mol/L·s O 7.6 × 10-5 mol/L·s O -5.0 x 105 mol/L-s A Moving to another question will save this response. MacBook Air F6 F5 吕口 F4 F3 F2 F1 #3 24 % 7 6. 4. 2 00
Consider the following complex reaction: P + 2Q → Products whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [P](M) [Q](M) Rate(M/s) 1 0.100 0.050 2.25 × 10−3 2 0.100 0.150 6.75 × 10−3 3 0.200 0.050 9.00 × 10−3 A) Write the rate law for this reaction. Use k to represent the rate constant. B) Solve for k in the above rate law (express your answer to three significant figures), and select the units for k.
2A(g) + 3/2B(g) Experiment e b) D d) k= 12345 Initial rate (mol/L.s) →→ C(g) 0.25*10-4 2.25x10-4 0.50×10-4 1.00×10-4 0.75*10-4 Initial [A] (mol/L) 5x10-2 15x10-2 5x10-2 10×10-2 5x10-2 unit: Overall reaction order is Rate = K[A][B] Initial [B] (mol/L) Reaction order with respect to A is Reaction order with respect to B is 5x10-2 5x10-2 10x10-2 5x10-2 15x10-2 O " O Calculate rate constant (k) based on data from experiment 3:
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4. The following data were obtained for the follwing chemical reaction: 2A + 3B ---> 2C + D Initial [A] Initial [B] Initial Rate of Formation Trial # (mmol/L) (mmol/L) of D (mmol/L*s) 1 4.0 6.0 1.60 2 2.0 6.0 0.80 3 4.0 3.0 0.40 (a) Determine the rate law equation for this reaction. Show your reasoning. (b) Find the rate constant, k, with units.
Following experimental data were obtained for the general reaction 20 + D→A + 2B Trial Concentration of C (M) Concentration of D (M) Initial Rate (M/s) 1 0.150 0.150 8.00x10-3 2 0.150 0.300 1.60x10-2 3 0.300 0.150 3.20x10-2 (a) Which trials do you select to find the order with respect to A? (b) The order of the reaction with respect to A is (c) Which trials do you select to find the order with respect to B? (d) The order of the reaction with respect to B is (e) The overall order of the reaction is (f) The value of the rate constant is