Asked by LS
Chemistry Equilibrium Constant PLEASE Help!?
In an experiment, equal volumes of 0.00150 M FeCl3 and 0.00150 M NaSCN were mixed together and reacted according to the equation:
Fe3+ (aq) + SCN– (aq) <--> Fe(SCN)2+ (aq)
The equilibrium concentration of FeSCN 2+(aq) was 2.70*10^-4
Calculate the equilibrium constant for this reaction.
In an experiment, equal volumes of 0.00150 M FeCl3 and 0.00150 M NaSCN were mixed together and reacted according to the equation:
Fe3+ (aq) + SCN– (aq) <--> Fe(SCN)2+ (aq)
The equilibrium concentration of FeSCN 2+(aq) was 2.70*10^-4
Calculate the equilibrium constant for this reaction.
Answers
Answered by
DrBob222
.......Fe^3+ + SCN^- ==> FeSCN^2+
I.....0.0015..0.0015......0
C.......-x.......-x.......x
E...0.0015-x..0.0015-x.....x
x = 2.70E-4
0.0015-x = ?
I.....0.0015..0.0015......0
C.......-x.......-x.......x
E...0.0015-x..0.0015-x.....x
x = 2.70E-4
0.0015-x = ?
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