Electrochemistry Cell Reactions and Equations

The video tutorial by the Science Chef introduces the Nernst equation, explaining its significance in calculating the electromotive force (EMF) of galvanic cells under both standard and non-standard conditions. The tutorial covers the equation's components, including the product quotient, and provides detailed examples of EMF calculations for zinc-nickel, magnesium-silver, and tin-copper half cells. The video concludes with a preview of the next tutorial on electrolysis.

What is the primary reason for using the Nernst Equation in electrochemistry?

• To calculate the standard EMF of a cell

• To determine the temperature of a reaction

• To measure the EMF of a cell under non-standard conditions

• To find the concentration of solid reactants

Which variable in the Nernst Equation represents the number of moles of electrons transferred?

• n, the number of moles of electrons

• T, the temperature in Kelvin

• F, Faraday's constant

• R, the molar gas constant

In the Nernst Equation, what does the reaction quotient (Q) represent?

• The ratio of the concentrations of products to reactants

• The temperature of the reaction

• The standard EMF of the cell

• The pressure of the system

What is the standard EMF of a cell made from zinc and nickel half-cells?

• 0.51 volts

• 0.53 volts

• 0.25 volts

• 0.76 volts

How many moles of electrons are transferred in the zinc and nickel cell reaction?

• Three

• Two

• Four

• One

What is the non-standard EMF of the cell made from magnesium and silver half-cells?

• 3.18 volts

• 3.21 volts

• 0.80 volts

• 2.38 volts

In the magnesium and silver cell, which metal acts as the anode?

• Zinc

• Copper

• Magnesium

• Silver

What is the non-standard EMF of the cell made from tin and copper half-cells?

• 0.34 volts

• 0.52 volts

• 0.15 volts

• 0.49 volts

How many moles of electrons are transferred in the tin and copper cell reaction?

• One

• Four

• Two

• Three

What is the calculated concentration of copper ions in the tin and copper cell?

• 0.52 molar

• 1.0 molar

• 0.0103 molar

• 0.001 molar