For a lab we constructed an electrochemical cell that consists of two compartments; one consisting of a zinc electrode submersed in a 0.15 M zinc chloride solution (the anode) and another consisting of a platinum electrode submersed in a solution that is 0.5 M in both potassium ferrocyanide (K4Fe(CN)6•3H2O) and potassium ferricyanide (K3Fe(CN)6) (the cathode). I need to calculate Q for the reaction.
From what I understand, the representation of the cell is as follows:
Zn
(s) | Zn
2+aq(0.15M) || Fe(CN)
63-(aq)(0.10 M), Fe(CN)
64-(aq)(0.10 M) | Pt
And the overall reaction is as follows:
Zn
(s) + 2Fe(CN)
64-(aq) Zn
2+aq + 2Fe(CN)
63-(aq)Am I right to say that the reaction quotient for this reaction is equal to:
Q = [Zn
2+]*[Fe(CN)
63-]
2/[Fe(CN)
64-]
2 = (0.15 M)(0.10 M)
2/(0.10 M)
2 = 0.15
The lab manual states that activities can be ignored. Thanks in advance.