Practice Problem: Cell Potential, Equilibrium Constants, and Free Energy Change

The video tutorial explains how to calculate cell potential (Ecell), equilibrium constant (K), and standard free energy change for a given electrochemical reaction. It provides a step-by-step guide to using reduction potentials to find Ecell, which is then used to determine K and the standard free energy change. The tutorial emphasizes the importance of using the correct values and expressions for accurate calculations.

What is the reduction potential for silver plus ions?

• 0.447 volts

• -0.7996 volts

• 0.7996 volts

• -0.447 volts

How is the cell potential (Ecell) calculated?

• E cathode plus E anode

• E anode minus E cathode

• E cathode minus E anode

• E anode plus E cathode

Which substance is reduced at the cathode?

• Solid silver

• Iron ions

• Silver ions

• Solid iron

What is the equilibrium constant (K) for the given reaction?

• 1.247

• 42.1

• 10^42.1

• 1.34 * 10^42

How many moles of electrons are transferred in the reaction?

• One

• Four

• Three

• Two

What is Faraday's constant value used in the calculation?

• 42.1

• 240.6 kilojoules per mole

• 1.247 volts

• 96,485 joules per mole volts

What is the standard free energy change in kilojoules per mole?

• 240.6 kJ/mol

• -2.406 kJ/mol

• -240.6 kJ/mol

• 2.406 kJ/mol