The resulting solution was allowed to attain equilibrium at 24C. The absorbance of the equilibrium solution was recorded, and the [FeSCN2+] was determined graphically to be 7.53 x 10^-5 M.
a)calculate number of moles of Fe3+ initially added to the solution
b)calculate number of moles of FeSCN2+ formed in the solution at equilibrium
c)calculate final number of moles of Fe3+ present in the solution after equilibrium
d)calculate concentration of Fe3+ in the solution at equilibrium
2007-03-05 02:57:45 · 2 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
a) Moles of Fe3+ = 5x10^-3 x 2 x 10^-3 = 10^-5
How can [FeSCN2+] = 7.53 x 10^-5 M ?
2007-03-05 03:08:02 · answer #1 · answered by ag_iitkgp 7 · 0⤊ 0⤋
Fe(NO3)3 + 3KSCN --> Fe(SCN)3 + 3KNO3
That has to be the reaction.
a) 5ml * (0.002mole Fe/liter)*(liter/1000ml) = 1 * 10^-5
b) moles KSCN added =
3ml* 0.02/1000 = 6 * 10^-5 (excess) so Fe is limiting
so max moles Fe(SCN)3 at eq = 1 * 10-5
but you said you got 7.53 times that!
c) same as b
d) same as b
2007-03-05 11:25:01 · answer #2 · answered by Dr Dave P 7 · 0⤊ 0⤋