In: Chemistry
Given the following information
Ag+(aq) + e- ↔ Ag(s) Eºred = 0.799 V
Ag2CrO4(s) + 2e- ↔ 2Ag(s) + CrO42-(aq) Eºred = 0.450 V
Determine the equilibrium constant at 25 °C for the reaction below:
Ag2CrO4(s) ↔ 2Ag+(aq) + CrO42-(aq)
1. |
9 × 10-18 |
|
2. |
1.6 × 10-12 |
|
3. |
1.2 × 10-6 |
|
4. |
1.6 × 1015 |
|
5. |
1.7 × 1039 |
Examine the following half reactions and select the strongest oxidizing agent among the species listed.
Cr2+(aq) + 2e- ↔ Cr(s) Eºred = -0.913 V
Sr2+(aq) + 2e- ↔ Sr(s) Eºred = -2.89 V
Fe2+(aq) + 2e- ↔ Fe(s) Eºred = -0.447 V
Co2+(aq) + 2e- ↔ Co(s) Eºred = -0.28 V
1. |
Cr2+(aq) |
|
2. |
Fe(s) |
|
3. |
Fe2+(aq) |
|
4. |
Sr2+(aq) |
|
5. |
Co2+(aq) |
2 points
QUESTION 5
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. |