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a student mixes 5.00 mL of 0.0020 M Fe(NO3)3 with 5.00 mL of.0020 KSCN solution at a certain temperature. He places a smaple ofthe resulting solution in a spectrometer, and measures thetransmittance as 37% at 447 nm.

a. What are the initial concentrations of FE and SCN

b. What are the final concentrations of FE, SCN, and FeSCN?

c. What is the measured value of Keq? PLEASE EXPLAIN STEPS FOR ALL POINTS WHICH I WILL GLADLY REWARD IFUNDERSTOOD< THANK YOU

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Deanna Hettinger
Deanna HettingerLv2
28 Sep 2019

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Related questions

Help please!

A student mixes 5.00 mL of 0.0020 M Fe(NO3)3 with 4.00 mL of 0.0020 M KSCN solution and 1.00 mL water at a certain temperature. He places a sample of the resulting solution in a spectrometer, and measures the transmittance as 31% at 447 nm.

a) What are the initial concentration of [Fe3+] and [SCN-]?

b) What are the final concentrations of [Fe3+], [SCN-], and [FeSCN2+]?

c) What is the measured value of Keq?

The molar absorptivity at 447 nm (ε = 4400). Path length = 1 cm.

Fe+3 + SCN- <===> FeSCN+2


You mix the following:

Volume of KSCN solution________ 4.35 mL

Original concentration of KSCN solution_________ 0.00321 M

Volume of ferric ion solution ________4.87 mL

Original concentration of ferric ion solution_________ 0.03753M

Voluume of distilled water _______5.25 mL


You measure the %T of the blank and sample at 447 nm using thesame cuvet. Only FeSCN2+ absorbs

at 446 nm! KSCN and Fe+3 are transparent.

%T of blank _____101.7

%T of sample_____ 49.1

constant [Molarity FeSCN2+ per absorbance]______ 0.001756M/A

********NOTE: This constant is only for this pre-lab*******


Calculate:

a) Millimoles of SCN- originally put in solution _______________mmoles

b) Millimoles of Fe+3 originally put in solution _______________mmoles

c) Total volume of solution _______________ mL

d) Molarity of FeSCN2+ at equilibrium _______________ M

e) Millimoles of FeSCN2+ at equilibrium _______________mmoles

f) Molarity of SCN- at equilibrium _______________ M

g) Molarity of Fe+3 at equilibrium _______________ M

h) Calculated equilibrium constant _______________


so far i found that

a)=0.0140 mmol

b)=0.183 mmol

c)=14.47 mL


i know that i have to use and ICE chart but i am not sure on howto calculate the change in moles from the reactants to theproducts?

if i do (0.014 - x) for the KSCN and (0.183 - x) fot theFe^3+and (0+x) for the FeSCN^+2 i have nothing to set it equal to?that what i dont understand

a chem 1515 student does the same experiment as the one you will be conducting this week but at a different temperature. She mixes 5.00 mL of 1.00 x 10-3 M solution of Fe(NO3)3 with 5.00 mL of 1.00 x 10-3 M KSCN solution. She finds out the equilibrium concentration of FeSCN2+ at theis condition to be 2.5 x 10-5 M. What is the value of the equilibrium constant for the reaction? Fe3+ (aq) + SCN- (aq) <--> FeSCN2+ (aq)

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