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Chapter 7: Problem 11

Fill in the blanks. During electrolysis of molten \(\mathrm{PbBr}_{2}\), ___ fumes are liberated at the anode.

Short Answer

Expert verified
Answer: Bromine gas fumes.

Step by step solution

01

Understanding Electrolysis

Electrolysis is a process in which an electric current is used to drive a non-spontaneous redox reaction. In this case, we are given a molten \(\mathrm{PbBr}_{2}\) compound undergoing electrolysis. In electrolysis, oxidation events happen at the anode, while reduction events occur at the cathode.
02

Find the ions present in molten PbBr2

Molten \(\mathrm{PbBr}_{2}\) is a liquid, and consists of ions. The ions present will be the cations \(\mathrm{Pb}^{2+}\) and anions \(\mathrm{Br}^{-}\), since \(\mathrm{PbBr}_{2}\) dissociate into its constituent ions when in molten state.
03

Determine the reactions happening at the Anode

At the anode during electrolysis, the oxidation reaction will take place. The anode is negatively charged and as a result it will attract the negatively charged ions, that is, the bromide ions (\(\mathrm{Br^{-}}\)). Bromide ions will be oxidized into bromine gas. The oxidation half-reaction can be written as: \(\mathrm{2Br^{-}} \rightarrow \mathrm{Br}_{2} + 2 e^{-}\)
04

Determine the fumes liberated at the Anode

Now, we can see that the anode produces \(\mathrm{Br}_{2}\) gas in the oxidation half-reaction. So, the fumes liberated in the electrolysis of molten \(\mathrm{PbBr}_{2}\) at the anode are: Bromine gas fumes.

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Most popular questions from this chapter

The standard electrode potentials of the electrodes are given below. Arrange them in decreasing order of ease of oxidation. (1) Electrode \(-\mathrm{I}, \mathrm{E}^{\circ}=-2.89 \mathrm{~V}\) (2) Electrode - II, E \(^{\circ}=-0.16 \mathrm{~V}\) (3) Electrode \(-\mathrm{III}, \mathrm{E}^{\circ}=0.77 \mathrm{~V}\) (4) Electrode \(-\mathrm{IV}, \mathrm{E}^{\circ}=-2.93 \mathrm{~V}\) (5) Electrode \(-\mathrm{V}, \mathrm{E}^{\circ}=-1.67 \mathrm{~V}\) (a) 32514 (b) 41523 (c) 35142 (d) 32145

State whether the following statements are true or false. The negative sign of the reduction potential indicates that reduction occurs at that electrode when connected to the standard hydrogen electrode.

State whether the following statements are true or false. During electrolysis, cations move towards the positive terminal.

In a voltaic cell, if iron and silver electrodes are connected with each other then current flows (a) from iron to silver outside the cell (b) from silver to iron within the cell (c) from silver to iron outside the cell (d) current does not flow in this cell

In the electroplating of iron by nickel, nickel sulphate solution is taken as an electrolyte. What is the acid that is added to the electrolyte during the process? (a) \(\mathrm{HCl}\) (b) \(\mathrm{HCN}\) (c) \(\mathrm{HNO}_{3}\) (d) \(\mathrm{H}_{2} \mathrm{SO}_{4}\)
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