The decomposition of nitrosyl bromide at 10 °C NOBR NO+½ Br, is second order in NOBr. In one experiment, when the initial concentration of NOBR was 0.187 M, the concentration of NOBR dropped to 5.16x10 M after 11.9 seconds had passed. Based on these data, the rate constant for the reaction is M's.

The decomposition of nitrosyl bromide at 10 °C NOBR NO+½ Br, is second order in NOBr. In one experiment, when the initial concentration of NOBR was 0.187 M, the concentration of NOBR dropped to 5.16x10 M after 11.9 seconds had passed. Based on these data, the rate constant for the reaction is M's.

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

The decomposition of nitramide in aqueous solution at 25 °C NH,NO,(aq)→N,0(g) + H,0(I) is first order in NH,NO,. During one experiment it was found that when the initial concentration of NH, NO, was 0.302 M, the concentration of NH,NO, dropped to 0.0507 M after 24805.0 s had passed. Based on this experiment, the rate constant for the reaction is
The decomposition of N,O5 to NO, and O, is first order, with a rate constant of 4.80 x 1o4/s at 45°C. If the initial concentration of N,O5 is 4.18×102 mol/L, what is the concentration of N205 after 548 s? How long would it take for the concentration ofN,O5 to decrease to 1.00 x 10-2 mol/L from an initial concentration of 4.18x102 mol/L?
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.
The decomposition of aqueous hydrogen peroxide (H2O2) to gaseous oxygen and water is a 1st order process. If it takes 6.0 h for the concentration of H2O2 to decrease from 0.40 M to 0.20 M, how many hours are required for the concentration to decrease from 0.70 M to 0.35 M?
The reaction, A → products, is known to be second order with respect to the concentration of A and second order overall. The rate constant for the reaction is 0.0500 M-1·min-1 at a certain temperature.If the initial concentration of A is 0.650 M. What will the concentration of A be after 40.0 min?How long would it take for 45.0% of the starting material (A) to undergo reaction?
The reaction A → B + C is found to be zero order. If it takes 4.2 102 seconds for an initial concentration of A to go from 0.58 M to 0.29 M, what is the rate constant for the reaction?
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0092 M-s : 2 HI (g) - H, (g) +L, (g) Suppose a 450. mL flask is charged under these conditions with 150. mmol of hydrogen iodide. After how much time is there only 75.0 mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. dlo x10 8. 미
The decomposition of ethylene oxide (CH₂)₂O(g) → CH₄(g) + CO(g) is a first order reaction with a half-life of 58.0 min at 652 K. The activation energy of the reaction is 218 kJ/mol. Calculate the half-life at 613 K.
The first-order decomposition of cyclopropane has a rate constant of 6.7 x 104 s1. If the initial concentration of cyclopropane is 1.33 M, what is the concentration of cyclopropane after 644 s? 0.15 M 0.86 M O 0.94 M 0.43 M 0.67 M