The solutions and concentrations are: 3.00 mL of 0.200 M Fe(NO3)3 and 2.00 mL of 0.375...
The solutions and concentrations are:
3.00 mL of 0.200 M Fe(NO3)3 and 2.00 mL of 0.375 M KSCN.
a) We are going to fill in the values for the first two rows of the RICE Table (or ICE-box). The change must be represented by a small letter "x" and must show the sign. So answers could be similar to -x, +x, 0, +2x, etc.
R: Fe^3+, SCN^-, FeSCN^-
I: __, __, __
C: __, __, __
E: -------------
b) You spec-200 gave you a concentration for the FeSCN2+ of 0.105 mol/L at equilibrium.
What is the value of x?
c) Now we are going to fill in the last row of the RICE Table (or ICE-box).
lar to -x, +x, 0, +2x, etc.
R: Fe^3+, SCN^-, FeSCN^-
I: --------
C: --------
E: __, __, __
d) Given these concentrations at equilibrium, what do you calculate the equilibrium constant for this reaction to be?
Please help! Thank you!
Homework Answers
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The solutions and concentrations are:
3.00 mL of 0.200 M Fe(NO3)3 and
2.00 mL of 0.375...
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