The following initial rate data are for the reaction of ICI with hydrogen: 21C1+ H₂12₂+ 2HCl Experiment [IC]. M [H₂lo. M 0.203 0.0655 0.406 0.0655 0.203 0.131 0.406 0.131 1 2 3 4 Rate 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 fa or 1. 4 k Submit Answer M2.8-1 Initial Rate, M-s-1 0.00151 Retry Entire Group 0.00301 0.00603 0.0121 9 more group attempts remaining

The following initial rate data are for the reaction of ICI with hydrogen: 21C1+ H₂12₂+ 2HCl Experiment [IC]. M [H₂lo. M 0.203 0.0655 0.406 0.0655 0.203 0.131 0.406 0.131 1 2 3 4 Rate 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 fa or 1. 4 k Submit Answer M2.8-1 Initial Rate, M-s-1 0.00151 Retry Entire Group 0.00301 0.00603 0.0121 9 more group attempts remaining

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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Evaluate the following data to determine whether the reaction is first or second order. Calculate the rate constant and be certain to give its unit. A → Product A (mmol/L) Time (sec) 1.00 0 0.50 11 0.25 20 0.10 48 0.05 105
The following initial rate data are for the reaction of ICI with hydrogen: 2 ICI + H2- →I2 + 2 HCI Experiment [ICI],, M [H2]o, M Initial Rate, M s-1 1 0.339 7.80x10-2 |3.63х10-3 0.678 7.80x10-2 7.26x10-3 3 0.339 0.156 1.45x10-2 14 0.678 0.156 2.90x10-2 Complete the rate law for this reaction in the box below. Use the form k[A]m[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. Rate = From these data, the rate constant is M-2s-1.
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The rate of a reaction is monitored by measuring the number of moles of product that form per liter per second. The data obtained are listed in the table below. Using this data, mathematically determine the order with respect to each reactant, the overall order of the reaction, determine the rate constant, k, with units, and write the complete rate law. Experiment [X], M [Y], M Rate, Msec-1 1 0.0500 0.0850 0.643 2 0.0300 0.0850 0.386
The following data was collected for the reaction 2 Mg + O2 --> 2MgO Determine the order for each reactant and write the rate law. Trial [Mg] (mol/L) [O2] (mol/L) Measured Rate(M/s) 1 .10 .10 2.0x10-3 2 .20 .10 4.0x10-3 3 .10 .20 8.0x10-3 According to this data the order for Mg is Answer (enter a number).
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For a reaction in which A and B react to form C, the following initial rate data were obtained: Initial Rate of [A] [B] Formation of C (mol/L) (mol/L) (mol/L's) 0.10 0.10 1.00 0.10 0.20 4.00 0.20 0.20 8.00 What is the rate law? A. Rate=k[A]°[B] B. Rate=k[A][B]? C. Rate=k[A]°[B]? D. Rate=k[A]3 E. Rate=k[A][B] Reset Selection
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The following initial rate data are for the reaction of ICl with hydrogen: 2 ICI + H Iz + 2 HCI Initial Rate, Ms! 1.57x10-2 3.13×10-2 6.24x10-2 0.125 Experiment [ICI]. M H), M 1 0.207 0.211 2 0.414 0.211 3 0.207 0.421 4 0.414 0.421 Complete the rate law for this reaction in the box below. Use the form k[A]"[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