values if needed for this question.The gas phase decomposition of hydrogen peroxide at 400 °CH202(g)H20(g) + ½ 02(g)is second order in H,02 with a rate constant of 0.650 M-1 s-1.If the initial concentration of H202 is 0.178 M, the concentration of H202 will beM after 49.0 seconds have passed. The rearrangement of ammonium cyanate to urea in aqueous solution at 50 °CNHẠNCO(aq)–→(NH2)2CO(aq)is second order in NH4NCO.In one experiment, when the initial concentration of NH4NCO was 0.874 M, the concentration ofNH4NCO dropped to 0.102 M after 506 minutes had passed.Based on these data, the rate constant for the reaction isM-1 min-1.

Answered: Image /qna-images/answer/6ce12847-d41a-453d-8363-0913e9d9c6e5.jpg

this question. The gas phase decomposition of hydrogen peroxide at 400 °C H202(g)H20(g) + ½ 02(g) is second order in H202 with a rate constant of 0.650 M-1 s-1. If the initial concentration of H202 is 0.178 M, the concentration of H202 will be M after 49.0 seconds have passed

this question. The gas phase decomposition of hydrogen peroxide at 400 °C H202(g)H20(g) + ½ 02(g) is second order in H202 with a rate constant of 0.650 M-1 s-1. If the initial concentration of H202 is 0.178 M, the concentration of H202 will be M after 49.0 seconds have passed

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

In a first order decomposition in which the rate constant is 0.0287 sec-1, how long will it take (in seconds) until 0.193 mol/L of the compound is left, if there was 0.985 mol/L at the start?
The decomposition of nitramide in aqueous solution at 25 °C NH₂ NO₂ (aq) → N₂O(g)+ H₂O(1) is first order in NH₂ NO2 with a rate constant of -1 4.70 × 10-5 S-¹ If the initial concentration of NH₂NO2 is 0.864 M, the concentration of NH₂ NO2 will be M after 32118 s have passed.
Hydrogen iodide decomposes slowly to H2 and I2 at 600 K. The reaction is second order in HI, and the rate constant is 9.7×10−6M−1s−1. If the initial concentration of HI is 0.100 M. What is its molarity after a reaction time of 7.00 days? What is the time (in days) when the HI concentration reaches a value of 0.080 M?
The decomposition of nitramide in aqueous solution at 25 °CNH2NO2(aq)N2O(g) + H2O(l)is first order in NH2NO2 with a rate constant of 4.70×10-5 s-1.If the initial concentration of NH2NO2 is 0.814 M, the concentration of NH2NO2 will be 0.227 M after s have passed.
The decomposition of C2H5Cl is first order. If the initial concentration of C2H5Cl is 2.50 M and after 706 s the concentration of C2H5Cl is found to be 2.000 M what is the numerical value of the first order rate constant, k in s-1, for the decomposition of C2H5Cl in decimal form? Thanks for the studying help
The decomposition of nitramide in aqueous solution at 25 °C NH2NO2(aq)–N20(g) + H20(1) is first order in NH,NO2 with a rate constant of 0.0000470 s1. If the initial concentration of NH2NO2 is 0.548 M, the concentration of NH2NO2 will be 0.0986 M after s have passed.
The decomposition of nitrous oxide at 565 °CN2O(g)N2(g) + ½ O2(g)is second order in N2O with a rate constant of 1.10×10-3 M-1 s-1.If the initial concentration of N2O is 2.22 M, the concentration of N2O will be 0.258 M after seconds have passed.
The dimerization of acetylene: 2C2H2 yields C4H4 is a second order. In one study, at 800 K, it was found that if [C2H2]=.400 M, the reaction occurs at a rate of 2.61 M/min. In another experiment, the reaction proceeds at 800 K with an initial concentration of 0.850M . What will the concentration of acetylene be at t=4.00 min? a) 0.0590 M b) 0.0676 M c)66.7 M d) 0.0150 M e)0.0367 M
Please don't provide handwritten solution ....
The decomposition of nitrous oxide at 565 °C N₂O(g) → N₂ (9)+½O₂(g) 1 is second order in N₂O with a rate constant of 1.10 × 10-³ M s If the initial concentration of N₂O is 2.16 M, the concentration of N₂O will be M after 1480 seconds have passed.
Solve it asap
At a certain temperature the rate of this reaction is second order in CICH₂CH₂Cl with a rate constant of 0.00455 M S -1 CICH₂CH₂Cl (g) → CH₂CHC1 (g) + HC1 (g) Suppose a vessel contains CICH₂CH₂Cl at a concentration of 1.11 M. Calculate the concentration of CICH₂CH₂Cl in the vessel 900. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.