is there a typo to this cell notation answer
Au(s)|AuCl4-(aq), Cl-(aq)|| F2(g)| F-(aq) |Pt(s)
If i look at the anode, should Cl- stay on the side of Au not AuCl4-
Au + 4Cl- yield AuCl4- + 3e
To determine whether there is a typo in the given cell notation, let's analyze the changes occurring at the anode and cathode during the electrochemical cell reaction.
First, let's break down the cell notation: Au(s)|AuCl4-(aq), Cl-(aq)|| F2(g)| F-(aq) |Pt(s)
Anode (left side): Au(s) is being oxidized due to the loss of electrons, so Au(s) → AuCl4-(aq) + 3e.
Cathode (right side): F2(g) is being reduced by gaining electrons, so F2(g) + 2e → 2F-(aq)
Now let's see if there might be a typo in the anode reaction: Au(s) + 4Cl-(aq) → AuCl4-(aq) + 3e
Comparing this to the given reaction, it seems that there is a discrepancy in the number of chloride ions involved. The given reaction shows 4Cl-, whereas the reaction represented in the cell notation shows only one Cl-.
To resolve this discrepancy, it is important to know the stoichiometry of the reaction and verify the correct coefficients. The balanced equation for the anode reaction should be:
Au(s) + 3Cl-(aq) → AuCl3(aq) + 3e
Considering this balanced equation, the correct cell notation should be:
Au(s)|AuCl3(aq), Cl-(aq)|| F2(g)| F-(aq) |Pt(s)
Therefore, it seems like there was indeed a typo in the cell notation, and Cl- should stay on the side of Au rather than AuCl4-.