A student mixes 5.00 mL 2.00x10-3 M FeCl3 with 3.00 mL 2.00x10-3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2+ is 1.28x10-4 M. Find Keq for the reaction a. Find the number of moles Fe3+ initially present. b. Find the number of moles SCN- initially present. c. What is the volume of the equilibrium mixture? d. How many moles of FeSCN2+ are in the equilibrium mixture?
A student mixes 5.00 mL 2.00x10-3 M FeCl3 with 3.00 mL 2.00x10-3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2+ is 1.28x10-4 M. Find Keq for the reaction a. Find the number of moles Fe3+ initially present. b. Find the number of moles SCN- initially present. c. What is the volume of the equilibrium mixture? d. How many moles of FeSCN2+ are in the equilibrium mixture?
Chemical Principles in the Laboratory
11th Edition
ISBN:9781305264434
Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Chapter23: Determination Of The Equilibrium Constant For A Chemical Reaction
Section: Chapter Questions
Problem 1ASA
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A student mixes 5.00 mL 2.00x10-3 M FeCl3 with 3.00 mL 2.00x10-3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2+ is 1.28x10-4 M. Find Keq for the reaction
a. Find the number of moles Fe3+ initially present.
b. Find the number of moles SCN- initially present.
c. What is the volume of the equilibrium mixture?
d. How many moles of FeSCN2+ are in the equilibrium mixture?
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