Consider a working voltaic cell based on the following redox reaction:    

If a reaction has a  ΔG = 0, this indicates that:

A 0.085 M solution of acetic acid (CH3COOH)  has a pH of 2.55. What is the percent ionization of this solution?

For the elementary reaction 2 NO (g)   →   N2O2(g)     the molecularity of the reaction is                           , and the rate law is, rate =                         .

Consider the following aqueous reaction between ammonia (NH3) and formic acid (HCOOH): NH4+ (aq)  + HCOO─ (aq)   ⇌    NH3 (aq)  +  HCOOH (aq)   Identify the stronger acid and predict whether the equilibrium lies to the left or to the right? Hint: The Ka of HCOOH is 1.8 x 10─4 Hint: The Ka of NH4+ is 5.5 x 10─10

A 0.025 M solution of acetic acid (CH3COOH)  has a pH of 2.98. What is the percent ionization of this solution?

Which of the following solutions will have the highest pH? Hint: This is not a calculation problem. Consider the type of acid and base (strong vs. weak acid and base).  

Copper metal, Cu (s), is produced by running a current through a solution of Cu2+ in an electrolytic cell. How many grams of copper metal can be deposited from Cu²⁺(aq) when a current of 2.50 A is run for 2.00 h? Hint:  F = 96,500 C/mol e− Hint:  1 A = 1 C/s

Consider the reaction of elemental bromine with elemental chlorine to make a bromochloride compound at 600 K:                                        2 BrCl(g)   ⇌   Br2(g)  +  Cl2(g)         KP = 81.0 A closed vessel at 600 K is charged with 3.00 atm of BrCl initially and allowed to reach equilibrium. What is the partial pressure of the Br2 (in atm) at that equilibrium?

Consider the pH curve when acetic acid (CH3COOH) is titrated with sodium hydroxide (NaOH):   What specie(s) are predominately present at point D in this titration?