5.) Consider the following equilibrium: Fe3+(aq) + SCN"(aq) = FESCN2+(aq) Initial concentrations: [Fe3+] = 0.150; [SCN] = 0.315; [FESCN2+] = 0 The equilibrium concentration of [FESCN2+]eg = 0.115 M. What is the numerical value of Kc for this equilibrium?

5.) Consider the following equilibrium: Fe3+(aq) + SCN"(aq) = FESCN2+(aq) Initial concentrations: [Fe3+] = 0.150; [SCN] = 0.315; [FESCN2+] = 0 The equilibrium concentration of [FESCN2+]eg = 0.115 M. What is the numerical value of Kc for this equilibrium?

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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Please don't provide handwritten solution ....
A student determines [FeSCN2+] is 0.00016 M at equilibrium. If the initial concentration of Fe3+ was 0.00080 M and the initial SCN- concentration was 0.0012 M, what is the measured value of Kc?
the equilibrium constant (K) is a quantitative measurement of theextent to which a chemical or physical reaction proceeds to completion. If two reactants ofknown initial concentration are mixed and then the concentrations of the products aremeasured once equilibrium has been established, then the equilibrium constant can becalculated using an ICE table.In this experiment you will measure the equilibrium constant for the formation of iron(III)thiocyanate from the iron(III) cation and thiocyanate anion:Fe3+(aq) + SCN-(aq) FeSCN2+(aq)The product, FeSCN2+, is intensely red, which means that its concentration can be measured byusing an ultraviolet-visible (UV-vis) spectrophotometer. So long as a solution is not tooconcentrated, the absorption of light at a particular wavelength by a chemical species isdescribed by Beer’s Law:A = εℓ[X] where A = absorption of light (unitless number)ε = molar absorptivity constant (cm-1 M-1)ℓ = path length (cm)[X] = concentration (M)The path length for our…
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In an aqueous chloride solution cobalt(I1) exists in equilibrium with the complex ion CoCl,2, Co2*(aq) is pink and CoCl,2"(aq) is blue. At Low Temperature the pink color predominates. At High Temperature the blue color is strong. If we represent the equilibrium as: Co?*(aq) + 4CI (aq)= CoCl," (aq) We can conclude that: J1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. 2. When the temperature is increased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. 3. When the temperature is increased the equilibrium concentration of Co2*: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question.
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Consider a receptor (R) that binds two ligands (L & M ) in a sequential fashion. For example, ligand "L" must be present before ligand "M" can bind. In dissociation reactions, it would look like this. R•L•M R•L + M with equilibrium constant Kam R•L OR+L with equilibrium constant Ka a. Derive an equation that relates the fraction [R•L•M]/[R]tot to the concentrations of free L and free M. b. In terms of the dissociation constant, Kam, what concentration of ligand "M" will lead to 50% of the receptor existing in the R•L•M state when [L] = 10 x Ka?
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