Question

1. Given the following information

   Ag⁺(aq) + e^- ↔ Ag(s)   Eº_red = 0.799 V

   Ag₂CrO₄(s) + 2e^- ↔ 2Ag(s) + CrO₄^2-(aq) Eº_red = 0.450 V

   Determine the equilibrium constant at 25 °C for the reaction below:

   Ag₂CrO₄(s) ↔ 2Ag⁺(aq) + CrO₄^2-(aq)

   	1.	9 × 10-18
   	2.	1.6 × 10-12
   	3.	1.2 × 10-6
   	4.	1.6 × 1015
   	5.	1.7 × 1039

1. Examine the following half reactions and select the strongest oxidizing agent among the species listed.

   Cr²⁺(aq) + 2e^- ↔ Cr(s) Eº_red = -0.913 V

   Sr²⁺(aq) + 2e^- ↔ Sr(s) Eº_red = -2.89 V

   Fe²⁺(aq) + 2e^- ↔ Fe(s) Eº_red = -0.447 V

   Co²⁺(aq) + 2e^- ↔ Co(s) Eº_red = -0.28 V

   	1.	Cr2+(aq)
   	2.	Fe(s)
   	3.	Fe2+(aq)
   	4.	Sr2+(aq)
   	5.	Co2+(aq)

2 points   

QUESTION 5

1. Which of the changes below will increase the voltage of the following cell?

   Co | Co²⁺ (0.010M) || H⁺ (0.010 M) | H₂(0.50 atm) | Pt

   	1.	Increase the pressure of H2 from 0.50 atm to 1.0 atm
   	2.	Increase the concentration of H+ from 0.010 to 0.050 M.
   	3.	Increase the mass of Co electrode from 12 grams to 15 g.
   	4.	Increase the concentration of Co2+ from 0.010 M to 0.40 M.

Answer 1