Understanding Cell Voltage and Standard Reduction Potentials

What is the significance of a more positive standard reduction potential?

• It means the reaction is non-spontaneous.

• It shows the reaction will not occur.

• It suggests a higher likelihood of reduction.

• It indicates a higher likelihood of oxidation.

Which formula is used to calculate cell voltage from standard electrode potentials?

• E° cell = E° anode - E° cathode

• E° cell = E° cathode + E° anode

• E° cell = E° cathode - E° anode

• E° cell = E° anode + E° cathode

What must be true for a reaction to be spontaneous in terms of E° cell?

• E° cell must be positive.

• E° cell must be zero.

• E° cell must be negative.

• E° cell must be less than zero.

What is the first step in calculating cell voltage?

• Add the half-equations together.

• Multiply the half-equations.

• Reverse the half-equations.

• Write down the two possible reduction half-equations.

Why should E° values not be multiplied when balancing equations?

• They are only used for oxidation reactions.

• They change with temperature.

• They are innate properties and do not depend on molarity.

• They depend on the number of moles.

In the zinc and silver reaction example, which metal acts as the active metal?

• Neither

• Both

• Silver

• Zinc

What is the calculated cell voltage for the zinc and silver reaction?

• 1.00 V

• 0.46 V

• 0.76 V

• 1.56 V

In the copper and silver reaction, which metal is the cathode?

• Both

• Silver

• Neither

• Copper

What is the cell voltage for the copper and silver reaction?

• 0.34 V

• 0.80 V

• 0.46 V

• 1.56 V

What is the purpose of breaking a complete equation into two halves?

• To identify the anode and cathode reactions.

• To calculate the pressure of the reaction.

• To determine the temperature of the reaction.

• To simplify the calculation of molarity.