Electrolysis: แบบฝึกหัด

In electrolysis, what is the correct name for a positively charged ion?

During the electrolysis of dilute sulfuric acid using platinum electrodes, which gas is produced at the cathode and in what volume ratio to the gas produced at the anode?

Which of the following statements correctly classifies the reactions at the electrodes during the electrolysis of any electrolyte?

Which statement explains why ionic compounds, such as sodium chloride, can conduct electricity when molten but not when solid?

A student investigates the electrolysis of aqueous sodium chloride. Which of the following observations and conclusions is correct for the anode?

Explain why ionic compounds, such as sodium chloride, can conduct electricity when in aqueous solution but not when in the solid state.

Write the ionic half-equation for the formation of oxygen gas at the anode during the electrolysis of dilute sulfuric acid.

During the electrolysis of concentrated sodium chloride solution, hydrogen gas is produced at the cathode instead of sodium. Explain this observation in terms of the reactivity of the elements involved and state whether the reduction of hydrogen ions is an oxidation or reduction process.

A student investigates the electrolysis of molten lead(II) bromide using inert graphite electrodes in a laboratory experiment. During the process, a reddish-brown gas is observed at the positive electrode and a silvery liquid forms at the negative electrode.

(a) State the name given to the negative electrode.

(b) Identify the silvery liquid formed at the negative electrode.

(c) Write the ionic half-equation, including state symbols, for the reaction occurring at the positive electrode.

Electrolysis is a process that uses electrical energy to bring about chemical changes in molten or aqueous ionic compounds.

Consider the electrolysis of molten lead(II) bromide, \( \text{PbBr}_2 \).

a) Identify the ions present in molten lead(II) bromide and explain why it conducts electricity in this state.

b) Predict the product formed at the positive electrode (anode) and the negative electrode (cathode).

c) Write a balanced half-equation for the reaction that occurs at each electrode.