Unit 9: Applications of Thermodynamics

A galvanic (voltaic) cell has a positive E°cell. This means the reaction is:

For a reaction with ΔH° = +100 kJ and ΔS° = +250 J/(mol·K), above what temperature (in K) does the reaction become spontaneous?

Calculate ΔG° (in kJ) for a cell with E°cell = 1.10 V and n = 2. Use F = 96485 C/mol. Round to the nearest whole number.

A reaction is spontaneous when

For a certain reaction at 298 K, ΔH° = -40 kJ and ΔS° = -120 J/K. At what temperature (in K) does this reaction change from spontaneous to nonspontaneous?

For a galvanic (voltaic) cell, which statement is true?

Given: Zn²⁺ + 2e⁻ → Zn, E° = -0.76 V and Cu²⁺ + 2e⁻ → Cu, E° = +0.34 V. The standard cell potential for the galvanic cell Zn|Zn²⁺||Cu²⁺|Cu is

Which process always has a positive entropy change (ΔS > 0)?

In electrolysis of aqueous NaCl, the products at the cathode and anode are

The relationship between the equilibrium constant K and the standard Gibbs free energy change is given by ΔG° = -RT ln K. If K = 1, then ΔG° is

A reaction is spontaneous when:

An electrochemical cell with a positive standard cell potential ([math]):

In an electrolytic cell:

The relationship [math] shows that:

Entropy increases when:

A reaction that is both exothermic and increases entropy:

Faraday's law of electrolysis relates:

In a galvanic (voltaic) cell:

The second law of thermodynamics states that:

At what temperature does this reaction become spontaneous?