Balancing Redox Reactions and Galvanic Cells

The video tutorial covers the preparation and study of galvanic cells, focusing on redox reactions and the calculation of cell potential using the Nernst equation. It explains the lab setup, including the use of a salt bridge and voltmeter, and details the process of measuring and calculating cell potential. The tutorial also emphasizes lab safety and proper cleanup procedures.

What is the main purpose of using the Nernst equation in the experiment?

• To determine the color change in the reaction

• To calculate the voltage produced by chemical cells

• To find the mass of the electrodes

• To measure the temperature of the solution

What happens to iron in the redox reaction with copper ions?

• It gains electrons and becomes Fe3+

• It loses electrons and becomes Fe2+

• It remains unchanged

• It forms a solid layer on copper

In a galvanic cell, where does oxidation occur?

• At the anode

• At the cathode

• In the voltmeter

• In the salt bridge

What is the function of a salt bridge in a galvanic cell?

• To prevent electron flow

• To act as a catalyst

• To allow ion migration between solutions

• To increase the cell potential

What is the role of the standard hydrogen electrode in measuring cell potential?

• It increases the reaction rate

• It acts as a catalyst

• It provides a reference potential of zero volts

• It absorbs excess electrons

Why must oxidation-reduction reactions be balanced?

• To ensure equal mass on both sides

• To maintain the same temperature

• To keep the solutions clear

• To have an equal number of electrons transferred

Which method involves subtracting the reduction potentials of the cathode and anode?

• The fourth method

• The second method

• The first method

• The third method

What should be done if all voltmeter readings are negative during the experiment?

• Add more solution

• Replace the electrodes

• Switch the connections of the wires to the voltmeter

• Increase the temperature

What is the significance of a positive voltmeter reading in the experiment?

• It suggests a need for more reactants

• It means the reaction is complete

• It shows a spontaneous reaction

• It indicates a non-spontaneous reaction

What should be done with the solutions after the experiment?

• Pour them down the drain

• Store them for future use

• Mix them with other chemicals

• Dispose of them in the appropriate waste container