in a study of the decomposition of hydrogen iodide on a gold surface at 150 °C HI(g)% H2(g) +½ I½(g) the concentration of HI was followed as a function of time. It was found that a graph of [HI] versus time in seconds gave a straight line with a slope of -1.58×104 M s and a y-intercept of 0.495 M. Based on this plot, the reaction is order in HI and the rate constant for the reaction is Ms!.

in a study of the decomposition of hydrogen iodide on a gold surface at 150 °C HI(g)% H2(g) +½ I½(g) the concentration of HI was followed as a function of time. It was found that a graph of [HI] versus time in seconds gave a straight line with a slope of -1.58×104 M s and a y-intercept of 0.495 M. Based on this plot, the reaction is order in HI and the rate constant for the reaction is Ms!.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter13: Electrochemistry

Section: Chapter Questions

Problem 13.90PAE: A chemical engineering student is studying the effect of pH on the corrosion of iron. Ellie...

See similar textbooks

Similar questions

For the reaction 2N2O5(g)4NO2(g)+O2(g) the following data were collected, where Rate=[N2O5]t Time (s) T = 338 K [N2O5] T=318K [N2O5] 0 1.00 101 M 1.00 101 M 100. 6.14 102 M 9.54 102 M 300 2.33 102 M 8.63 102 M 600. 5.41 1O3 M 7.43 102 M 900. 1.26 1O3 M 6.39 102 M Calculate Ea for tills reaction.
A chemical engineering student is studying the effect of pH on the corrosion of iron. Ellie following data are collected: Corrosion Rate (mm/year) ph 0.03 13.00 0.06 12.00 0.16 11.00 0.22 10.00 0.25 9.00 0.25 8.00 0.25 7.00 0.25 6.00 0.25 5.00 0.27 4.00 0.37 3.00 0.38 2.80 0.63 2.80 1.00 2.80 Plot corrosion rate vs. pH. (HINT: Label the x axis with decreasing pH.) (a) How would you describe the dependence of corrosion on pH? (b) When the pH goes below 3, bubbles appear in the solution. What change takes place in the reduction half-reaction at low pH? (c) How do you explain the shape of the curve at the lowest pH? (Based on a graph in the Kirk-Otbmer Encyclopedia of Chemical Technology, 4th ed., vol 7. New York: John Wiley & Sons, p. 559.)
In a study of the gas phase decomposition of nitrosyl chloride at 400 K NOC(gNO(g) + ½ Cl2(g) the concentration of NOCI was followed as a function of time. It was found that a graph of 1/[NOCI] versus time in seconds gave a straight line with a slope of 7.97x10-4 M sl and a y-intercept of 38.0 M!. Based on this plot, the reaction is | order in NOCI and the rate constant for the reaction is
For the reaction of the ammonium ion with nitrous acid, the net reaction is NH4*(aq) + HNO2(aq) → N2(g) + 2H2O() + H*(aq) If the initial concentration of nitrous acid is 1.00 M and, after 28.8 s has elapsed, the concentration of nitrous acid has fallen to 0.82 M, what is the average rate of the reaction over this time interval? 0.0063 M/s 0.028 M/s -0.0063 M/s -0.028 M/s O 0.063 M/s
(Self-test 17A.1) Predict how the total pressure varies during the gas-phase reaction 2NOBr(g) → 2NO(g) + Br:(g) in a constant volume container at constant temperature. Define it in terms of a (fraction of NOBr reacted) and po (initial total pressure).
Please highlight the answers you found or underline them
1) if a plot of In(k) v.s 1/T of this pesticide showed a straight line with an equation of the line Y = -0.0356 X +0.0005. Calculate the activation energy of this reaction in (kJ/mol) 2) calculate the equilibrium concentration of the reactants and of the products 3) find how long it will take to reach the equilibrium
In a study of the decomposition of hydrogen iodide on a gold surface at 150 °C HI(g)% H2(g) + ½ I½(g) the concentration of HI was followed as a function of time. It was found that a graph of [HI] versus time in seconds gave a straight line with a slope of -1.91×10-4 Ms and a y-intercept of 0.235 M. Based on this plot, the reaction is reaction is order in HI and the rate constant for the Ms!
а. Identify THREE (3) isotherm shapes that are typically encountered in an adsorption process for a single adsorbate and illustrate the behavior through equilibrium relations.
Present the equations, calculations for solving kinetic problems. The chart can be made using a spreadsheet or by hand. Calculate the activation energy for the cementation of copper by iron, from the copper sulfate solution containing 1.3 g Cu/L, having obtained the following data: T (C) 85 75 65 55 45 kx 105 3,9 3,1 2,5 1,9 1.5 (cm/s)
9. The following reaction 2 N₂O5(g) → 4 NO₂(g) + O₂(g) was studied at several temperatures, and the following values of k were obtained: k (S-1) 2.0 X 105 7.3 X 10.5 2.7 x 104 9.1 x 104 2.9 X 103 Using linear regression and the techniques developed in this lab, calculate the activation energy and collision frequency for this reaction. T(°C) 20.0 30.0 40.0 50.0 60.0 10. Using the data from question 9, find k at 100°C.
The decomposition reaction of atmospheric peroxyacetylnitrate (PAN) to products was studied, and the following rates were obtained. Temperature, "C Rate constant, s 00 5.60 x 10 10.0 3.20 x 10 20.0 1.60 x 10 30.0 7.60 - 10 Fit this data into the Arrhenius equation. Give the values of the following: Slope = Select ] y-intercept [ Select Pearson coetficient (R) Select] activation energy of this reaction in k/mol | Select) collision frequency factor A= Select