We can use the Nernst equation to find E from Q and vice versa. Therefore, if you know the Ksp of a salt, you can use it to find the cell potential. Imagine a concentration cell in which one half-cell has a silver electrode in a saturated solution of Ag2SO4 and the other half-cell is a silver electrode in a 0.5 M solution of AGNO3. Use 310 K as the temperature, F = 96485 C/mol, R = 8.314 J/ mol K 1. Given that Ksp of silver sulphate is 1.2 x 10-5, what is the concentration of Ag+ in the saturated solution? 2. The cell notation can be written as: Ag(S) || Ag+(aq) (saturated conc.) || Ag+ (aq) (0.5M) || Ag(s) Use the Nernst equation to solve for Ecell under these conditions. 3. Write the chemical equation for the precipitation of A92SO4, and use Ksp to solve for Delta G°

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-Please answer all 5 questions:
We can use the Nernst equation to find E from Q and vice versa. Therefore, if
you know the
Ksp of a salt, you can use it to find the cell potential. Imagine a concentration
cell in which
one half-cell has a silver electrode in a saturated solution of Ag2SO4 and the
other half-cel
is a silver electrode in a 0.5 M solution of AGNO3.
Use 310 K as the temperature, F = 96485 C/mol, R = 8.314 J/ mol K
1. Given that Ksp of silver sulphate is 1.2 x 10-5, what is the concentration of
Ag+ in the
saturated solution?
2. The cell notation can be written as:
Ag(S) || Ag+(aq) (saturated conc.) || Ag+ (aq) (0.5M) || Ag(s)
Use the Nernst equation to solve for Ecell under these conditions.
3. Write the chemical equation for the precipitation of A92SO4, and use Ksp to
solve for
Delta G°
4. Using the thermodynamic values given, calculate Delta H° and Delta S° for
the precipitation
reaction at 310 K.
Delta H° kJ/mol. Delta S° J/mol-K
Ag+ (ag). 105. 78
S042- (aa). -909. 25.1
AgaS04 (s). -716. 203
5. At what temperature does the spontaneity reverse? If there isn't a
temperature at
which this occurs, explain why not.
Transcribed Image Text:Chemistry -Please answer all 5 questions: We can use the Nernst equation to find E from Q and vice versa. Therefore, if you know the Ksp of a salt, you can use it to find the cell potential. Imagine a concentration cell in which one half-cell has a silver electrode in a saturated solution of Ag2SO4 and the other half-cel is a silver electrode in a 0.5 M solution of AGNO3. Use 310 K as the temperature, F = 96485 C/mol, R = 8.314 J/ mol K 1. Given that Ksp of silver sulphate is 1.2 x 10-5, what is the concentration of Ag+ in the saturated solution? 2. The cell notation can be written as: Ag(S) || Ag+(aq) (saturated conc.) || Ag+ (aq) (0.5M) || Ag(s) Use the Nernst equation to solve for Ecell under these conditions. 3. Write the chemical equation for the precipitation of A92SO4, and use Ksp to solve for Delta G° 4. Using the thermodynamic values given, calculate Delta H° and Delta S° for the precipitation reaction at 310 K. Delta H° kJ/mol. Delta S° J/mol-K Ag+ (ag). 105. 78 S042- (aa). -909. 25.1 AgaS04 (s). -716. 203 5. At what temperature does the spontaneity reverse? If there isn't a temperature at which this occurs, explain why not.
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