How do you build Q for a cell reaction?

• Reactants over products with no powers
• Products over reactants, each raised to its stoichiometric power
• Molar masses over charges, each times n

What is the Nernst equation for a cell potential E?

• E equals E standard minus R T over n F times ln Q
• E equals E standard plus n F over R T times Q
• E equals R T over F times Q minus E standard

Both electrodes use the same metal but the ion amounts differ on the two sides and a voltage appears. What is this cell?

• A dry cell at standard state
• A cell at equilibrium
• A concentration cell

E standard for a cell is positive. What does that say about K?

• K sits below 1 and reactants dominate
• K sits above 1 and products dominate
• K equals 1 and E stays zero

In a concentration cell, which way does each half cell run?

• Oxidation in the dilute half cell, reduction in the concentrated one
• Reduction in the dilute half cell, oxidation in the concentrated one
• Oxidation in both half cells until Q equals zero

Concentrations work in Q only when the solution is dilute.

A running cell shows its voltage fading toward zero. What does that say about Q?

• Q is approaching K as the cell nears equilibrium
• Q has drifted far from K toward zero
• Q now holds activities instead of concentrations

Two cells share the same concentration ratio, but one moves one electron and the other moves two. How do their voltages compare?

• Both give the same voltage
• The two-electron cell gives the larger voltage
• The two-electron cell gives the smaller voltage