[1 minute = 60 seconds] A. Nature of Reactants A.1 The Affect of Metal Degradation Based on Acid Type Four acids are put into vary test tubes and magnesium metal [Mg] is dropped into each test tube and the time it takes for the metal to completely dissolve is measured: Lab Data Test Tube-1 (H,SO, 3M) time: 3.68seconds Test Tube-2 (HC1 6M) time: 4.25seconds Test Tube-3 (CH COOH 6M) time: 17.58 minutes/seconds Test Tube-4 (H3PO.): 5.54 minutes/seconds %3D Question-1: Calculate the reaction rates for each tube utilizing the equation (use the concentration of each respective acid): Rate= A[X]/time(s)

[1 minute = 60 seconds] A. Nature of Reactants A.1 The Affect of Metal Degradation Based on Acid Type Four acids are put into vary test tubes and magnesium metal [Mg] is dropped into each test tube and the time it takes for the metal to completely dissolve is measured: Lab Data Test Tube-1 (H,SO, 3M) time: 3.68seconds Test Tube-2 (HC1 6M) time: 4.25seconds Test Tube-3 (CH COOH 6M) time: 17.58 minutes/seconds Test Tube-4 (H3PO.): 5.54 minutes/seconds %3D Question-1: Calculate the reaction rates for each tube utilizing the equation (use the concentration of each respective acid): Rate= A[X]/time(s)

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...

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For the reduction 2FeCl3 + SnCl2 =====➔ 2 FeCl2 + SnCl4 in aqueous solution the following data were obtained at 25oC t(min) 1 3 7 11 40 Y 0.01434 0.02664 0.03612 0.04102 0.05058 Where y is the amount of FeCl3 reacted in moles per liter. The initial concentrations of SnCl3 and FeCl3 were respectively, 0.03125, 0.0625 moles/L. a.)Show that the reaction is third order (derive the rate law), and b.) calculate the average specific rate constant.
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Determine the rate law, rate constant(k) of the reaction with the given information. What's the balanced reaction using the half-reaction method. Also for experiment 1 what will be the concentration of [Fe2+] after 10 seconds? Chart Shows the initial reaction rate measurement for the acidic conditions performed in acidic condition (H+). Equation 2Fe2+(aq)+Cl2(aq)----> 2Fe3+(aq)+2Cl-(aq) Experiments [Fe2+] [Cl2] [H+] Rate Experiment 1 0.0014 M 0.0045 M 0.10 M 1.03x10-5 M/s Experiment 2 0.0040 M 0.0045 M 0.10 M 1.98x10-5 M/s Experiment 3 0.0014 M 0.0090 M 0.10 M 2.02x10-5 M/s Experiment 4 0.0040 M 0.0090 M 0.10 M 3.90x10-5 M/s Experiment 5 0.0014 M 0.0045 M 0.05 M 1.97x10-5 M/s Experiment 6 0.0014 M 0.0045 M 0.01 M 9.98x10-5 M/s
Reducing NO Emissions Adding NH3 to the stack gases at an electric power generating plant can reduceNOx emissions. This selective noncatalytic reduction (SNR) process depends on the reaction between NH3 (an odd-electron compound) and NO.$$4NH3(g)+6NO(g)5N2(g)+6H2O(g)The following kinetic data were collected at 1200 K. Experiment [NH3] (M) [NO] (M) Rate (M/s) 1 1.00x10-5 1.00x10-5 0.120 2 2.00x10-5 1.00x10-5 0.240 3 2.00x10-5 1.50x10-5 0.360 4 2.50x10-5 1.50x10-5 0.450 What is the rate-law expression for the reaction? Do not add multiplication symbols to your answer. $$Rate=
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The manganese(II)-catalyzed redox reaction between cerium(IV) and thallium(I) is thought to proceed by a three-step mechanism: Ce4+(aq) + Mn2+(aq) --> Ce3+(aq) + Mn3+(aq) (slow)Ce4+(aq) + Mn3+(aq) --> Ce3+(aq) + Mn4+(aq)Mn4+(aq) + Tl+(aq) --> Mn2+(aq) + Tl3+(aq) (a) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process. Rate = k [Mn2+] [Mn3+] Rate = k [Ce4+]2 Rate = k [Ce4+] [Tl+] Rate = k [Mn2+] [Ce4+] Rate = k [Ce4+]2 [Tl+] Rate = k [Mn3+] [Tl+]
The manganese(II)-catalyzed redox reaction between cerium(IV) and thallium(I) is thought to proceed by a three-step mechanism: Ce4+(aq) + Mn2+(aq) --> Ce3+(aq) + Mn3+(aq) (slow)Ce4+(aq) + Mn3+(aq) --> Ce3+(aq) + Mn4+(aq)Mn4+(aq) + Tl+(aq) --> Mn2+(aq) + Tl3+(aq) (a) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process. Rate = k [Mn2+] [Mn3+] Rate = k [Ce4+]2 Rate = k [Ce4+] [Tl+] Rate = k [Mn2+] [Ce4+] Rate = k [Ce4+]2 [Tl+] Rate = k [Mn3+] [Tl+] (b) Choose the correct chemical equation for the overall process. Ce4+(aq) + Mn2+(aq) --> Ce3+(aq) + Mn3+(aq) Ce4+(aq) + Mn3+(aq) --> Ce3+(aq) + Mn4+(aq) 2 Ce4+(aq) + Tl+(aq) --> 2 Ce3+(aq) + Tl3+(aq) (c) Identify an intermediate in the reaction. Mn2+ Ce3+ Mn3+ Ce4+ (d) Identify the catalyst in the reaction. Mn2+ Mn3+ Ce3+ Ce4+ (e) Identify a reactant in the reaction. Ce3+ Ce4+ Mn2+ Mn3+ (f) Identify a product in the reaction. Mn3+ Mn2+ Ce4+…
Given Zn(s)| Zn 2+ (aq) (1M) || Ag+2+ (aq) (1M) | Ag (s) Eocell = 1.562V What will the Ecell be if the [Zn2+] = 0.75M and [Ag+] =0.25 M at 40.00oC (313.15K)? The overall reaction is Zn(s) + 2 Ag+ (aq) --> 2 Ag (s) + Zn 2+ (aq) (Answer has 3 digits after the decimal)
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