The following initial rate data are for the reduction of nitric oxide with hydrogen: 2 NO + 2 H2 N2 + 2 H20 Experiment [NO]o, M [H2]o, M Initial Rate, M s-1 1 0.454 0.116 3.44x10-2 2 0.908 0.116 0.138 3 0.454 0.232 6.89x10-2 4 0.908 0,232 0.275 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n, where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is M-25-1.

The following initial rate data are for the reduction of nitric oxide with hydrogen: 2 NO + 2 H2 N2 + 2 H20 Experiment [NO]o, M [H2]o, M Initial Rate, M s-1 1 0.454 0.116 3.44x10-2 2 0.908 0.116 0.138 3 0.454 0.232 6.89x10-2 4 0.908 0,232 0.275 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n, where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is M-25-1.

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

Q2
The following results were obtained for the below reaction in experiments designed for the study of the rate of the reaction. A + B=> 2C Experiment Initial concentrations mol/L [A] [B] Rate of disappearance of A (M/sec) 1 0.030 0.030 2.0x10-3 2 0.030 0.060 4.0x10-3 4 0.060 0.030 4.0x10-3 Write the differential rate law for this reaction. What will be the initial rate of disappearance of A, if an experiment is attempted with A and B both equal to 0.060M? Write the integrated rate law for the concentration of A. Calculate the half-life for A Calculate the concentration of A in experiment 2 after 60 seconds rate constant = 2.22M^-1sec^-1
Chemistry please i need the answer of any two of them thanks.
The following initial rate data are for the oxidation of nitrogen monoxide by oxygen at 25 °C: 2 NO + 0,2 NO, [NO], M 6.66×10-3 1.33x10-2 6.66x10-3 1.33x10-2 [0-]o, M 2.20x10-3 2.20x10-3 4.40x10-3 4.40x10-3 Experiment Initial Rate, Ms 8.20x10-4 3.27x10-3 1.64x10-3 6.54x10-3 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]" , where 'l' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is
The following initial rate data are for the reduction of nitric oxide with hydrogen: ... 2 NO + 2 HzN2 + 2 H2O Experiment NO],, M [H]o, M Initial Rate, M s 8.66x10-2 1 0.370 0.408 2 0.740 0.370 0.740 0.408 0.816 0.346 0.173 0.693 3 0.816 From these data, what is the rate constant in M?s1 (A) 2.55 B) 1.55 (c) 3.55 D) 4.55
help me pleaseee
The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution: NH4+NO₂ → N₂ + 2 H₂O Experiment [NH4+]o, M [NO₂ ]o, M Initial Rate, M. s-1 0.0358 1.45 x 10-6 0.0715 0.0358 0.0715 1 2 3 4 Rate = 0.128 0.128 0.255 0.255 Complete the rate law for this reaction in the box below. Use the form k[A]" [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. k = 2.89 x 10-6 2.88 x 10-6 5.76 x 10-6 M-1.s-1
The following initial rate data are for the reaction of nitrogen monoxide with ozone at 25 °C: NO + 03 NO₂ + O₂ Experiment [NO]o, M [03]o, M Initial Rate, M-s1 0.192 0.0497 0.928 0.192 0.0994 1.86 0.384 0.0497 1.86 0.384 0.0994 3.71 1 2 3 4 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or 71. Rate = k= M
Use the following data table to answer the following questions. Experiment Concn. of A (M) Concn. of B (M) Initial rate (M/s) 1 0.10 0.010 1.2e-3 2 0.10 0.040 4.8e-3 3 0.20 0.010 2.4e-3 d. The rate constant of the reaction is e. The rate of reaction when concentration of A and B are 0.15M and 0.075M is
The following initial rate data are for the reaction of ICl with hydrogen:2 ICl + H2I2 + 2 HCl Experiment [ICl]o, M [H2]o, M Initial Rate, M s-1 1 0.113 3.10×10-2 1.81×10-4 2 0.226 3.10×10-2 3.63×10-4 3 0.113 6.20×10-2 7.25×10-4 4 0.226 6.20×10-2 1.45×10-3 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = k_____ From these data, the rate constant is ______M-2s-1.
The following initial rate data are for the reaction of ICl with hydrogen:2 ICl + H2I2 + 2 HCl Experiment [ICl]o, M [H2]o, M Initial Rate, M s-1 1 0.438 0.105 9.37×10-3 2 0.876 0.105 1.87×10-2 3 0.438 0.209 3.71×10-2 4 0.876 0.209 7.42×10-2 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = _______ From these data, the rate constant is __________M-2s-1.
The following initial rate data are for the oxidation of nitrogen monoxide by oxygen at 25 oC:2 NO + O22 NO2 Experiment [NO]o, M [O2]o, M Initial Rate, M s-1 1 9.78×10-3 1.69×10-3 1.41×10-3 2 1.96×10-2 1.69×10-3 5.68×10-3 3 9.78×10-3 3.38×10-3 2.83×10-3 4 1.96×10-2 3.38×10-3 1.14×10-2 Complete the rate law for this reaction in the box below.Use the form k[A]m[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = k[NO]2[O2] From these data, the rate constant is ____M-2s-1.