10) The following set of data was obtained by the method of initial rates for the reaction: > 10) BrO3-(aq) + 5 Br-(aq) + 6 H+(ag) – 3 Br2(aq) + 3 H20(1). Calculate the initial rate when BrO3- is 0.30 M, Br- is 0.050 M, and H+ is 0.15 M. Expt | [BrO3-], M| [Br-]M | [H+], M Rate, M/s 0.10 0.10 0.10 8.0 x 10-4 0.20 0.10 0.10 1.6 x 10-3 0.20 0.15 0.10 2.4 x 10-3 4 0.10 0.10 0.25 5.0 x 10-3 A) 6.1 × 10-5 M/s B) 2.7 × 10-3 M/s C) 5.3 × 10-2 M/s D) 8.4 × 10-2 M/s four (4) auestions: The relative initial rates of the reaction A2 + B2 - products in vess 1. 3.

10) The following set of data was obtained by the method of initial rates for the reaction: > 10) BrO3-(aq) + 5 Br-(aq) + 6 H+(ag) – 3 Br2(aq) + 3 H20(1). Calculate the initial rate when BrO3- is 0.30 M, Br- is 0.050 M, and H+ is 0.15 M. Expt | [BrO3-], M| [Br-]M | [H+], M Rate, M/s 0.10 0.10 0.10 8.0 x 10-4 0.20 0.10 0.10 1.6 x 10-3 0.20 0.15 0.10 2.4 x 10-3 4 0.10 0.10 0.25 5.0 x 10-3 A) 6.1 × 10-5 M/s B) 2.7 × 10-3 M/s C) 5.3 × 10-2 M/s D) 8.4 × 10-2 M/s four (4) auestions: The relative initial rates of the reaction A2 + B2 - products in vess 1. 3.

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...

See similar textbooks

Similar questions

I need help with all parts of this question:
For the reaction 4A(g) + 3B(g) → 2C(g) The following data were obtained at constant temperature: Experiment Initial [A](mol/L) Initial [B](mol/L) Initial Rate(mol/L · min) 1 0.100 0.100 5 2 0.300 0.100 45 3 0.100 0.200 10 4 0.300 0.200 90 Pick the best expression for the rate law for the reaction: k[A]2[B] Correct Calculate k (using the data from the table),
7.) The results of kinetics experiments have shown the rate of the following reaction:A + 2B + C ↓ products has the following rate law: rate = k[A]2[B]0[C]1with a rate constant of k = 1.3 × 10–4 L2/mole2·s (M –2·s–1).a.) What is the initial reaction rate if the initial concentrations of A, B, and C, are 0.2, 0.3, and 0.4 M, respectively?b.) What is the initial reaction rate if the initial concentrations of A, B, and C, are 0.2, 2.7, and 0.4 M, respectively?
13.74 Methyl acetate, CH,COOCH3, reacts in basic solu- tion to give acetate ion, CH;COO , and methanol, CH,OH. CH,COOCH,(ag) + OH (ag) → CH;COO (ag) + CH;OH(aq) The overall order of the reaction was determined by start- ing with methyl acetate and hydroxide ion at the same con- centrations, so [CH,COOCH3] = [OH]= x. Then Rate = k[CH,COOCH;"[OH¯]" = kx"*n %3D %3D Determine the overall order and the value of the rate con- stant by plotting the following data assuming first- and then second-order kinetics. Time (min) [CH,COOCH;] (mollL) 0.00 0.01000 3.00 0.00740 4.00 0.00683 5.00 0.00634 10.00 0.00463 20.00 0.00304 30.00 0.00224
17) For the following reaction give the expression for the average rate for each species in the equation. 3 Ag₂S(s) + Al(s) + 3 H₂O(1)→6 Ag(s) + Al₂O3(s) + 3 H₂S(aq)
4) Use the data below to determine the rate law and the value of k for the following reaction CHC13 (g) + Cl2 (9) → CC14 (g) + HCl (g) [CHCI3] (M) [Cl2] (M) Initial Rate 0.0035 Experiment 1 0.010 0.010 2 0.020 0.010 0.0069 3 0.020 0.020 0.0098 4 0.040 0.040 0.0270
In the presence of excess thiocyanate ion, SCN-, the following reaction is first order in iron(III) ion, Fe3+; the rate constant is 1.27/s. Fe3+(aq) + SCN-(aq) → Fe(SCN)2+(aq). How many seconds would be required for the initial concentration of Fe3+ to decrease to 12.5% of its initial value? Express your answer to two decijal positions.
In a study of the decomposition of hydrogen iodide on a gold surface at 150 °C HI(g)% H2(g) + ½ I½(g) the concentration of HI was followed as a function of time. It was found that a graph of [HI] versus time in seconds gave a straight line with a slope of -1.91×10-4 Ms and a y-intercept of 0.235 M. Based on this plot, the reaction is reaction is order in HI and the rate constant for the Ms!
Consider the reaction 5B1¯ (aq) + Br0, (aq) + 6H† (aq)→3B12 (aq) + 3H2O(1) The average rate of consumption of Br is 1.16×10-4 M/s over the first two minutes. What is the average rate of formation of Br2 during the same time interval? Express your answer with the appropriate units.
The gas phase decomposition of hydrogen iodide at 700 K HI(g)- →½ H2(g) + ½ I2(g) is second order in HI. In one experiment, when the initial concentration of HI was 2.23 M, the concentration of HI dropped to 0.656 M after 591 seconds had passed. Based on these data, the rate constant for the reaction is M-1 s-1.
An experiment was carried out to investigate the effect of concentration on the reaction: BrO3(aq) + 5 Br (aq) + 6 H* (aq) = 3 Br₂ (1) + 3 H₂O (1) The following data was obtained: Initial [BrO3] Initial [Br] Initial [H*] Initial Rate Trial (mol/L) (mol/L) (mol/L) (mol/L's) 1 0.10 0.10 0.10 8.0 x 10-4 2 0.20 0.10 0.10 1.6 x 10-3 3 0.20 0.20 0.10 3.2 x 10-3 4 0.10 0.10 0.20 3.2 x 10-3 a) Deduce and state the rate law equation for this reaction. Show your process/reasoning. b) Calculate the value of k, the rate constant with correct units.
Write rate law for the chemical reaction ?