NH3 1/2 N2 + 3/2 H₂the following data were obtained:[NH3], Mseconds2.33x10-31.17x10-35.85x10-42.93x10-40439660770Hint: It is not necessary to graph these data.(1)The observed half life for this reaction when the starting concentration is 2.33×10-3 M iswhen the starting concentration is 1.17×10-3 M isS.(2)The average rate of disappearance of NH3 from t = 0 s to t = 439 s isMs-1(3)The average rate of disappearance of NH3 from t = 439 s to t = 660 s isMs1(4)Based on these data, the rate constant for this zeroorder reaction isMs1s and

Half life is time for concentration to have. This can be easily seen from the table, concentration…

Answered: NH3 1/2 N2 + 3/2 H₂ the following data…

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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Calculate the half life when the rate is 6.2x10^-4
6) The decomposition of reactant R was studied, and the data given below was obtained at 100.0 °C: R> products time (min) concentration (M) 0.120 35.6 5.83 17.8 25.6 0.0910 0.060 0.046 0.030 a) What is the half-life of the reaction in minutes? Explain. b) Various plots of the concentration of the reactant versus time are given below. What is the order of the reaction? Explain. ILD is 20 time (min) time (min) 05 -35 time (min) c) What is the value of the rate constant at 100.0 °C? d) Would you expect the half-life of the reaction to be longer, shorter, or the same at 60.0 °C? Explain. e) The activation energy in the forward direction is 95.0 kl/mol, and the enthalpy change for the forward reaction is 30.0 kl/mol. Sketch the reaction coordinate diagram for this reaction. ERER AR
A certain first order reaction has a half-life of 56.0 s. How long will it take (in s) for the reactantconcentration to decrease from 6.50 M to 3.68 M? Give your answer to three sig figs
Pls helo ASAP. Pls help in all asked questions.
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.
I need help with questions 6-10 please
In a study of the gas phase decomposition of hydrogen iodide at 700 K HI(g)- →½ H2(g) + ½ I2(g) the following data were obtained: [HI], M seconds 1.48 0.740 0.370 0.185 750 2.25x103 5.25x103 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 1.48 M is 750 s and when the starting concentration is 0.740 M is 1500 S. (2) The average A(1/[HI]) / At from t = 0 s to t = 750 s is M-1 s-1. The average A(1/[HI]) / At from t 750 s to t = 2.25×103 s is M-1 s-1. (3) Based on these data, the rate constant for this 0 order reaction is M-1 s-1.
A particular reaction is proposed to be first order. What plot would support this conclusion? Periodic Table and Datasheet a linear plot of [reactant] versus time a linear plot of In [reactant] versus time an linear plot of [reactant]1 versus time O an exponential decay of In [reactant] versus time
* 97% 7:58 PM Wed Feb 12 х Unanswered •1 attempt left • Due on Feb 13 Rate law of a reaction is experimentally determined as Rate = k [A]^2 [B]^0 [C] The unit of k is sec/M 1/M^3-sec 1/M^2-secc. 1/M^4-sec M^3/sec Submit
In a study of the decomposition of nitrous oxide at 565 °C N2₂O(g) N₂(g) + ½ O₂(g) the following data were obtained: [N₂0], M seconds 0.750 0 0.375 1.50x10³ 0.188 4.47x10³ Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.750 M is concentration is 0.375 M is S. (2) The average A(1/[N₂0])/ At from t = 0 s to t = 1.50x10³ s is The average A(1/[N₂0])/ At from t = 1.50x10³ s to t = 4.47x103 s is (3) Based on these data, the rate constant for this 9.40×10-2 1.04x104 M-1 S-1. order reaction is M-1 S-1. M-¹ S-1. s and when the starting

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