25 Questions
What is the relationship between the moles of electrons and the product of current and time according to Faraday's Law?
Directly proportional
In an electrolytic cell, where does reduction occur?
Cathode
What is the value of Faraday's constant, F, in coulombs per mole of electrons?
96485 C/mol e-
How many moles of electrons are required to reduce 1 mole of calcium cations?
2 moles
In an electrochemical cell, which electrode does oxidation occur?
Anode
Which statement about electrodes in electrochemistry is true?
Inert electrodes do not change mass while the cell operates.
Which process occurs at the anode in an electrolytic cell?
Oxidation
According to Faraday's Law, the moles of electrons passed through a cell is calculated by which formula?
$\frac{\text{Current} \times \text{Time in seconds}}{96485}$
What is the purpose of using stoichiometry in electrochemical processes?
To determine mass of material plated/removed from solution.
If a constant current of 3 A flows through a cell for 2 hours, what can be determined using Faraday's Law?
The total charge transferred
In the given voltaic cell, what is the oxidation half-reaction at the anode?
Mg → Mg2+ + 2e-
What is the cell potential of the voltaic cell at 25°C?
+1.054 V
How many moles of electrons are transferred in the given voltaic cell?
2 moles
What does the reaction quotient (Q) represent in electrochemical cells?
The relative ratio of products to reactants
How does Faraday's Law relate to the process of electrolysis?
It quantifies the amount of substances produced at an electrode during electrolysis
Which electrode in a galvanic cell is responsible for the reduction of metal ions?
Cathode
In which electrode are electrons used up in an electrolytic cell?
Cathode
What is the function of the salt bridge in a voltaic cell?
Maintain electrical neutrality
When aluminum metal is oxidized to aluminum cation, which electrode is affected?
Anode
Which electrode gains mass by reducing copper(II) to copper metal in a galvanic cell?
Cathode
What effect does increasing the tin (II) ion concentration in the anode compartment have on the cell potential?
It decreases the cell potential.
If more hydrogen gas is added to the cathode compartment, what impact does this have on the cell potential?
It increases the cell potential.
What is the significance of adding more tin metal to the half-cell in terms of cell potential?
It has no effect on the cell potential.
How does increasing the tin (II) ion concentration compare to increasing the pressure of hydrogen gas in terms of their impact on cell potential?
One increases while the other decreases cell potential.
Which action among increasing tin (II) ion concentration, adding more hydrogen gas, and increasing tin metal will NOT change the measured cell potential?
Increasing tin metal
Learn about Faraday's law and electrolysis, where copper is reduced at the cathode and bromide is oxidized at the anode. Understand the relationship between moles of electrons and the product of current and time in electrochemical processes.
Make Your Own Quizzes and Flashcards
Convert your notes into interactive study material.
Get started for free
