After completing part II of the experiment, a student uses her calibration curve tofind that the equilibrium concentration of the product in one trial is 1.19x10 M. Ifthe "initial" concentrations of Fes+ and SCN in the reaction mixture are those givenbelow, what is the equilibrium concentration of Fe*, [Fe*]ea? Give your answer inmillimolar (mM) to three decimal places.3+3+1[SCN ]o= 6.18x10-4 M[Fe3+]o = 1.11x10-3 M%3D[FENCS2+]eg =1.19x10-4 M

We would first write a reaction between Fe3+ and SCN- to form product [FeNCS2+] , then we would…

After completing part II of the experiment, a student uses her calibration curve to find that the equilibrium concentration of the product in one trial is 1.19x10¯4 M. If the "initial" concentrations of Fet and SCN¯ in the reaction mixture are those given below, what is the equilibrium concentration of Fe*, [Fe*]eg? Give your answer in millimolar (mM) to three decimal places. [SCN ]0= 6.18x10-4 M [Fe3+lo = 1.11x10-3 M %3D [FENCS2+]eg = 1.19x10-4 M

After completing part II of the experiment, a student uses her calibration curve to find that the equilibrium concentration of the product in one trial is 1.19x10¯4 M. If the "initial" concentrations of Fet and SCN¯ in the reaction mixture are those given below, what is the equilibrium concentration of Fe, [Fe]eg? Give your answer in millimolar (mM) to three decimal places. [SCN ]0= 6.18x10-4 M [Fe3+lo = 1.11x10-3 M %3D [FENCS2+]eg = 1.19x10-4 M

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.35PAE: In the reaction in Exercise 12.33, another trial was carried out. The reaction began with an initial...

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In the reaction in Exercise 12.33, another trial was carried out. The reaction began with an initial concentration of N2 equal to the initial concentration of NO. Each had a concentration of 0.100 mol L-1. WTat were the equilibrium concentrations of all species? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) ^2 NO K = 4.1 X 10~4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L'1 ofO2, what were the equilibrium concentrations of all species?
Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?
Again the experiment in Exercise 12.33 was redesigned. This time, 0.15 mol each of N, and O2 was injected into a 5.0-L container at 2500 K, at which the equilibrium constant is 3.6 X 10-?. What was the composition of the reaction mixture at equilibrium? l'he following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) *2 2 NO K = 4.1 X IO-4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L-’ ofO2, what were the equilibrium concentrations of all species?
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7-29 The following reaction was allowed to reach equilibrium at 25°C. Under each component is its equilibrium concentration. Calculate the equilibrium constant, K, for this reaction.
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