Question 17.1: When chlorine gas is bubbled through an aqueous solution of ...

When chlorine gas is bubbled through an aqueous solution of NaBr, chloride ions and liquid bromine are the products of the spontaneous reaction. For this cell,
(a) Draw a sketch of the cell, labeling the anode, the cathode, and the direction of electron flow.
(b) Write the half-reaction that takes place at the anode and at the cathode.
(c) Write a balanced equation for the cell reaction.
(d) Write an abbreviated notation for the cell.

STRATEGY

1. Split the equation into two half-reactions.
2. Recall that the anode
• is where oxidation takes place.
• is the electrode toward which anions move.
• is where electrons are produced.
3. The cathode
• is where reduction takes place.
• is the electrode toward which cations move.
• is where electrons are released by the anode through an external circuit.

The blue check mark means that this solution has been answered and checked by an expert. This guarantees that the final answer is accurate.
Learn more on how we answer questions.
See Figure 17.4, where all the appropriate parts are labeled and the direction of electron
flow is indicated.

cathode:       Cl2(g) + 2e  2Cl(aq)Cl_{2}(g)  +  2e^{-}  →  2Cl^{-}(aq) (reduction)

anode:       2Br(aq)  Br2(l) + 2eBr^{-}(aq)  →  Br_{2}(l)  +  2e^{-} (oxidation)

Cl2(g) + 2Br(aq)  2Cl(aq) + Br2Cl_{2}(g)  +  2Br^{-}(aq)  →  2Cl^{-}(aq)  +  Br_{2}(l)

Pt | Br2Br_{2}, BrBr^{-} || ClCl^{-} | Cl2Cl_{2} | Pt

(a) Sketch of the cell

 

(b) Half-reactions

 

(c) Balanced equation

(d) Abbreviated cell notation

To summarize our discussion of the structure of voltaic cells,
• a voltaic cell consists of two half-cells. They are joined by an external electric circuit through which electrons move and a salt bridge through which ions move.
• each half-cell consists of an electrode dipping into a water solution. If a metal participates in the cell reaction, either as a product or as a reactant, it is ordinarily used as the electrode; otherwise, an inert electrode such as platinum is used.
• in one half-cell, oxidation occurs at the anode; in the other, reduction takes place at the cathode. The overall cell reaction is the sum of the half-reactions taking place at the anode and cathode.

fig 17.4

Related Answered Questions

Question: 17.5

Verified Answer:

ⓐ N: +5 → +2 reduction Ag: 0 → +1 oxidation 1....